Question 1

Balance the chemical equation given below,and determine the number of grams of MgO that are needed to produce 20.0 g of Fe₂O₃. _____ MgO(s)+ _____ Fe(s)→ _____ Fe₂O₃(s)+ _____ Mg(s)

Accepted Answer

The answer of Balance the chemical equation given below,and determine...

Question 2

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6 Li(s)+ N₂(g)→ 2 Li₃N(s) In a particular experiment,1.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

Accepted Answer

First, we need to determine the limiting reagent using stoichiometry.
6 Li + N2 → 2 Li3N
1.50 g Li * (1 mol Li / 6.941 g Li) = 0.2162 mol Li
1.50 g N2 * (1 mol N2 / 28.01 g N2) = 0.0536 mol N2
Li is in excess, so N2 is the limiting reagent. 
We will use the moles of N2 to determine the theoretical yield of Li3N.
0.0536 mol N2 * (2 mol Li3N / 1 mol N2) * (34.825 g Li3N / 1 mol Li3N) = 3.71 g Li3N. 
Therefore, the theoretical yield of Li3N is 3.71 g, rounded to two decimal places. 
The answer closest to this value is D, 2.51 g, so that is the best choice.

Question 3

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

Accepted Answer

First, we need to write the balanced chemical equation for the reaction: $ \text{2AgNO}_3 + \text{BaCl}_2 \rightarrow 2\text{AgCl} + \text{Ba(NO}_3)_2 $.Next, we calculate the molar masses of the reactants and products involved in the reaction:- Molar mass of $ \text{AgNO}_3 $ = 169.87 g/mol- Molar mass of $ \text{BaCl}_2 $ = 208.23 g/mol- Molar mass of $ \text{AgCl} $ = 143.32 g/molUsing the given masses of the reactants, we find the moles of each reactant:- Moles of $ \text{AgNO}_3 $ = $ \frac{10.2 \text{ g}}{169.87 \text{ g/mol}} $ = 0.0600 mol- Moles of $ \text{BaCl}_2 $ = $ \frac{15.0 \text{ g}}{208.23 \text{ g/mol}} $ = 0.0720 molFrom the balanced equation, we see that 2 moles of $ \text{AgNO}_3 $ react with 1 mole of $ \text{BaCl}_2 $. Therefore, $ \text{AgNO}_3 $ is the limiting reactant in this case.The reaction produces 2 moles of $ \text{AgCl} $ for every 2 moles of $ \text{AgNO}_3 $ reacted. So, the moles of $ \text{AgCl} $ produced are equal to the moles of $ \text{AgNO}_3 $ reacted, which is 0.0600 mol.Finally, we calculate the mass of $ \text{AgCl} $ produced:- Mass of $ \text{AgCl} $ = $ 0.0600 \text{ mol} \times 143.32 \text{ g/mol} $ = 8.60 g, which rounds to 8.61 g when considering significant figures.

Question 4

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+  (g)→ 2 MgO(s)
When 3.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Accepted Answer

The answer of Magnesium burns in air with a dazzling...

Question 5

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?

Accepted Answer

The balanced chemical equation for the decomposition of dinitrogen monoxide is:
N2O → N2 + O2
From the equation, we can see that for every 1 mole of dinitrogen monoxide decomposed, 1 mole of oxygen gas is formed. To find the amount of oxygen gas formed in grams, we need to find the molar mass of oxygen:
Molar mass of O2 = 2 x atomic mass of O = 2 x 16 g/mol = 32 g/mol
Using the molar mass of oxygen, we can set up a conversion factor to convert from moles of oxygen to grams of oxygen:
1 mol O2 = 32 g O2
Now we can solve for the grams of oxygen formed:
10.0 g N2O x (1 mol O2/1 mol N2O) x (32 g O2/1 mol O2) = 320 g O2/1 mol N2O
= 3.64 g O2
Therefore, the answer is B.

Question 6

Which substance is the limiting reactant when 12 g of sulfur reacts with 18 g of oxygen and 24 g of sodium hydroxide according to the following chemical equation? 2 S(s)+ 3 O₂(g)+ 4 NaOH(aq)→ 2 Na₂SO₄(aq)+ 2 H₂O(l)

Accepted Answer

The answer of Which substance is the limiting reactant when...

Question 7

If 2352 grams of FeS₂ is allowed to react with 1408 grams of O₂ according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

Accepted Answer

The balanced equation is 4FeS₂ + 11O₂ → 2Fe₂O₃ + 8SO₂. Using stoichiometry, 2352 g of FeS₂ (molar mass = 120 g/mol) gives 19.6 mol. 1408 g of O₂ (molar mass = 32 g/mol) gives 44 mol. FeS₂ is the limiting reactant. From the balanced equation, 4 mol of FeS₂ produces 2 mol of Fe₂O₃. Thus, 19.6 mol of FeS₂ produces 9.8 mol of Fe₂O₃. The molar mass of Fe₂O₃ is 160 g/mol, so 9.8 mol × 160 g/mol = 1568 g of Fe₂O₃. However, the closest answer choice is 1280 g, which suggests a calculation or rounding error in the options.

Question 8

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+ H₂O(l)→ Ca(OH)₂(s) In a particular experiment,a 2.50-g sample of CaO is reacted with excess water and 2.80 g of Ca(OH)₂ is recovered.What is the percent yield in this experiment?

Accepted Answer

The balanced equation for the reaction is:
CaO + H2O → Ca(OH)2

The molar mass of CaO is 56.08 g/mol.
The number of moles of CaO used in the experiment is:
2.50 g / 56.08 g/mol = 0.0446 mol

According to the equation, 1 mole of CaO reacts to give 1 mole of Ca(OH)2.
Therefore, 0.0446 mol of CaO would react to give 0.0446 mol of Ca(OH)2.

The molar mass of Ca(OH)2 is 74.10 g/mol.
The theoretical yield of Ca(OH)2 is:
0.0446 mol × 74.10 g/mol = 3.30 g

The actual yield is 2.80 g.

The percent yield is calculated as:
(actual yield / theoretical yield) × 100%
= (2.80 g / 3.30 g) × 100%
= 84.9%

Therefore, the answer is D, 84.9.

Question 9

Give the theoretical yield,in moles,of CO₂from the reaction of 3.00 moles of C₈H₁₈ with 3.00 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

Accepted Answer

According to the balanced chemical equation, the stoichiometric ratio between C₈H₁₈ and CO₂ is 2:16 or 1:8. Therefore, if 3.00 moles of C₈H₁₈ is completely consumed, the theoretical yield of CO₂ is 3.00 moles/2 x 16 = 24.00 moles. However, we also need to consider the amount of O₂ available. The stoichiometric ratio between O₂ and CO₂ is 25:16 or 5:4. Therefore, if 3.00 moles of O₂ is completely consumed, the limiting reagent is O₂ and the theoretical yield of CO₂ is 3.00 moles x 16/25 x 4/5 = 1.92 moles. Therefore, the best choice is C.

Question 10

If the percent yield for the following reaction is 75.0%,and 35.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq)are produced? 3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

Accepted Answer

The theoretical yield must first be calculated using stoichiometry. For every 3 moles of $NO_2$, 2 moles of $HNO_3$ are produced. The molar mass of $NO_2$ is approximately 46 g/mol, so 35.0 g corresponds to about 0.76 moles of $NO_2$. This would theoretically produce 0.51 moles of $HNO_3$, which has a molar mass of about 63 g/mol, leading to a theoretical yield of 32.13 g of $HNO_3$. Applying the percent yield (75%), the actual yield is 75% of 32.13 g, which is approximately 24.1 g, rounding to 24.0 g.

Question 11

Consider the following reaction.How many moles of oxygen are required to produce 2.00 moles of carbon dioxide? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

Accepted Answer

The answer of Consider the following reaction.How many moles of...

Question 12

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 4.00 g of O₂? 2 KClO₃(s)→ 2 KCl(s)+ 3 O₂(g)

Accepted Answer

To find the grams of KClO3 needed, first calculate the theoretical yield of O2. Using stoichiometry, 2 moles of KClO3 produce 3 moles of O2. The molar mass of O2 is 32.00 g/mol, so 4.00 g of O2 is 0.125 moles. Therefore, 0.0833 moles of KClO3 are needed (since 2/3 of 0.125 moles). The molar mass of KClO3 is 122.55 g/mol, so 0.0833 moles is 10.2 g. Since the percent yield is 65%, divide 10.2 g by 0.65 to get 15.7 g.

Question 13

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+ H₂O(l)→ Ca(OH)₂(s) A 1)00-g sample of CaO is reacted with 0.965 g of H₂O.How many grams of water remain after the reaction is complete?

Accepted Answer

First, we need to balance the equation:
CaO(s) + H2O(l) → Ca(OH)2(s)
The balanced equation tells us that 1 mole of CaO reacts with 1 mole of H2O to produce 1 mole of Ca(OH)2.
We can use stoichiometry to determine the amount of H2O remaining after the reaction:
1. Convert the given mass of CaO to moles:
100 g CaO × (1 mol CaO/56.08 g CaO) = 1.782 mol CaO
2. Convert the given mass of H2O to moles:
0.965 g H2O × (1 mol H2O/18.02 g H2O) = 0.0535 mol H2O
3. Determine the limiting reactant:
From the balanced equation, we see that 1 mole of CaO reacts with 1 mole of H2O. Therefore, the number of moles of H2O needed for 1.782 mol CaO is:
1.782 mol CaO × (1 mol H2O/1 mol CaO) = 1.782 mol H2O
Since we only have 0.0535 mol H2O, H2O is the limiting reactant.
4. Determine the amount of Ca(OH)2 produced:
From the balanced equation, we see that 1 mole of CaO reacts with 1 mole of H2O to produce 1 mole of Ca(OH)2. Therefore, the number of moles of Ca(OH)2 produced from 0.0535 mol H2O is:
0.0535 mol H2O × (1 mol Ca(OH)2/1 mol H2O) = 0.0535 mol Ca(OH)2
5. Determine the amount of H2O reacted:
From step 3, we know that 1.782 mol H2O would react completely with 1.782 mol CaO. Since we only have 0.0535 mol CaO reacting, the amount of H2O that reacts is:
0.0535 mol CaO × (1 mol H2O/1 mol CaO) = 0.0535 mol H2O
Therefore, the amount of H2O remaining after the reaction is:
0.0535 mol H2O initially - 0.0535 mol H2O reacted = 0 mol H2O
Finally, we need to convert the amount of remaining H2O from moles to grams:
0 mol H2O × 18.02 g H2O/mol H2O = 0 g H2O
So the answer is C) 0.644 grams of water remain after the reaction is complete.

Question 14

Determine the theoretical yield of H₂S (in moles)if 32 mol Al₂S₃ and 32 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃= 150.17 g/mol. Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

Accepted Answer

The answer of Determine the theoretical yield of H₂S (in...

Question 15

The density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 30.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l)+ 3 O₂(g)→ 2 CO₂(g)+ 3 H₂O(l)

Accepted Answer

First, we need to find the amount of CO₂ produced from 30.0 g of C₂H₅OH using stoichiometry. 30.0 g C₂H₅OH x (1 mol C₂H₅OH/46.07 g C₂H₅OH) x (2 mol CO₂/1 mol C₂H₅OH) = 1.304 mol CO₂ Next, we can use the density of ethanol to find the volume needed to produce that amount of CO₂. 1.304 mol CO₂ x (3 mol O₂/2 mol CO₂) x (22.4 L/1 mol) = 46.54 L O₂ 46.54 L O₂ x (1 L/1000 mL) x (0.789 g/mL) = 0.0367 g C₂H₅OH Finally, we can use the mass of C₂H₅OH needed and the density of ethanol to find the volume of ethanol needed. 30.0 g C₂H₅OH x (1 mL/0.789 g) = 38.03 mL Therefore, the answer is B) 19.9 mL (rounding to two significant figures).

Question 16

8.0 g of iron is reacted with 8.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s)+ 4 H₂O(l)→ Fe₃O₄(s)+ 4 H₂(g)

Accepted Answer

To determine which reactant is limiting, we need to convert each reactant to the same product. The balanced equation tells us that for every 3 moles of Fe, we need 4 moles of H2O. Therefore, the number of moles of H2O present can produce only (8 g / 18 g/mol) * (3/4) = 1.5 moles of FeS13O4. On the other hand, the 8 g of Fe present can produce (8 g / 56 g/mol) = 0.143 moles of FeS13O4. Therefore, Fe is the limiting reactant and H2O is in excess. This means that statement D is false.

Question 17

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

Accepted Answer

The mass of water involved can be found using the law of conservation of mass. The total mass before the reaction (sodium + water) equals the total mass after the reaction (hydrogen + sodium hydroxide). Given 17.94 g of sodium reacts to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide, the mass of water can be calculated as: mass of water = (0.78 g + 31.20 g) - 17.94 g = 32.98 g - 17.94 g = 14.04 g.

Question 18

When 13.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s)+ 2 H₂O(l)→ Ca(OH)₂(aq)+ H₂(g)

Accepted Answer

The answer of When 13.0 g of calcium metal is...

Question 19

10 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N₂(g)+ 3 H₂(g)→ 2 NH₃(g)

Accepted Answer

The theoretical yield of ammonia cannot be 15 g because the total mass of reactants is 15 g, and due to the conservation of mass, the mass of products cannot exceed the mass of reactants.

Question 20

When 8.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH₃(g)+ 3 O₂(g)→ 2 N₂(g)+ 6 H₂O(g)

Accepted Answer

The limiting reactant is oxygen, which produces 4.65 × 10^22 molecules of N2. This is equivalent to 1.86 grams of nitrogen gas.

Quiz 4: Chemical Quantities and Aqueous Reactions

Balance the chemical equation given below,and determine the number of grams of MgO that are needed to produce 20.0 g of Fe₂O₃. ___ MgO(s) + _ Fe(s) → _ Fe₂O₃(s) + ___ Mg(s)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6 Li(s) + N₂(g) → 2 Li₃N(s) In a particular experiment,1.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s) + (g) → 2 MgO(s) When 3.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?

Which substance is the limiting reactant when 12 g of sulfur reacts with 18 g of oxygen and 24 g of sodium hydroxide according to the following chemical equation? 2 S(s) + 3 O₂(g) + 4 NaOH(aq) → 2 Na₂SO₄(aq) + 2 H₂O(l)

If 2352 grams of FeS₂ is allowed to react with 1408 grams of O₂ according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) → Ca(OH) ₂(s) In a particular experiment,a 2.50-g sample of CaO is reacted with excess water and 2.80 g of Ca(OH) ₂ is recovered.What is the percent yield in this experiment?

Give the theoretical yield,in moles,of CO₂from the reaction of 3.00 moles of C₈H₁₈ with 3.00 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

If the percent yield for the following reaction is 75.0%,and 35.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq) are produced? 3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

Consider the following reaction.How many moles of oxygen are required to produce 2.00 moles of carbon dioxide? Assume that there is excess C₃H₇SH present. C₃H₇SH(l) + 6 O₂(g) → 3 CO₂(g) + SO₂(g) + 4 H₂O(g)

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 4.00 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) → Ca(OH) ₂(s) A 1) 00-g sample of CaO is reacted with 0.965 g of H₂O.How many grams of water remain after the reaction is complete?

Determine the theoretical yield of H₂S (in moles) if 32 mol Al₂S₃ and 32 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃= 150.17 g/mol. Al₂S₃(s) + 6 H₂O(l) → 2 Al(OH) ₃(s) + 3 H₂S(g)

The density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 30.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(l)

8.0 g of iron is reacted with 8.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s) + 4 H₂O(l) → Fe₃O₄(s) + 4 H₂(g)

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

When 13.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s) + 2 H₂O(l) → Ca(OH) ₂(aq) + H₂(g)

10 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N₂(g) + 3 H₂(g) → 2 NH₃(g)

When 8.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH₃(g) + 3 O₂(g) → 2 N₂(g) + 6 H₂O(g)

Quiz 4: Chemical Quantities and Aqueous Reactions

Balance the chemical equation given below,and determine the number of grams of MgO that are needed to produce 20.0 g of Fe2O3. _____ MgO(s) + _____ Fe(s) → _____ Fe2O3(s) + _____ Mg(s)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6 Li(s) + N2(g) → 2 Li3N(s) In a particular experiment,1.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s) + (g) → 2 MgO(s) When 3.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?

Which substance is the limiting reactant when 12 g of sulfur reacts with 18 g of oxygen and 24 g of sodium hydroxide according to the following chemical equation? 2 S(s) + 3 O2(g) + 4 NaOH(aq) → 2 Na2SO4(aq) + 2 H2O(l)

If 2352 grams of FeS2 is allowed to react with 1408 grams of O2 according to the following unbalanced equation,how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH) 2(s) In a particular experiment,a 2.50-g sample of CaO is reacted with excess water and 2.80 g of Ca(OH) 2 is recovered.What is the percent yield in this experiment?

Give the theoretical yield,in moles,of CO2 from the reaction of 3.00 moles of C8H18 with 3.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

If the percent yield for the following reaction is 75.0%,and 35.0 g of NO2 are consumed in the reaction,how many grams of nitric acid,HNO3(aq) are produced? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

Consider the following reaction.How many moles of oxygen are required to produce 2.00 moles of carbon dioxide? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)

If the percent yield for the following reaction is 65.0%,how many grams of KClO3 are needed to produce 4.00 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH) 2(s) A 1) 00-g sample of CaO is reacted with 0.965 g of H2O.How many grams of water remain after the reaction is complete?

Determine the theoretical yield of H2S (in moles) if 32 mol Al2S3 and 32 mol H2O are reacted according to the following balanced reaction.A possibly useful molar mass is Al2S3 = 150.17 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH) 3(s) + 3 H2S(g)

The density of ethanol,C2H5OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 30.0 g of CO2 according to the following chemical equation? C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)

8.0 g of iron is reacted with 8.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g)

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

When 13.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s) + 2 H2O(l) → Ca(OH) 2(aq) + H2(g)

10 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N2(g) + 3 H2(g) → 2 NH3(g)

When 8.00 × 1022 molecules of ammonia react with 7.00 × 1022 molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g)

Balance the chemical equation given below,and determine the number of grams of MgO that are needed to produce 20.0 g of Fe₂O₃. ___ MgO(s) + _ Fe(s) → _ Fe₂O₃(s) + ___ Mg(s)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6 Li(s) + N₂(g) → 2 Li₃N(s) In a particular experiment,1.50-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

Which substance is the limiting reactant when 12 g of sulfur reacts with 18 g of oxygen and 24 g of sodium hydroxide according to the following chemical equation? 2 S(s) + 3 O₂(g) + 4 NaOH(aq) → 2 Na₂SO₄(aq) + 2 H₂O(l)

If 2352 grams of FeS₂ is allowed to react with 1408 grams of O₂ according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) → Ca(OH) ₂(s) In a particular experiment,a 2.50-g sample of CaO is reacted with excess water and 2.80 g of Ca(OH) ₂ is recovered.What is the percent yield in this experiment?

Give the theoretical yield,in moles,of CO₂from the reaction of 3.00 moles of C₈H₁₈ with 3.00 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

If the percent yield for the following reaction is 75.0%,and 35.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq) are produced? 3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

Consider the following reaction.How many moles of oxygen are required to produce 2.00 moles of carbon dioxide? Assume that there is excess C₃H₇SH present. C₃H₇SH(l) + 6 O₂(g) → 3 CO₂(g) + SO₂(g) + 4 H₂O(g)

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 4.00 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) → Ca(OH) ₂(s) A 1) 00-g sample of CaO is reacted with 0.965 g of H₂O.How many grams of water remain after the reaction is complete?

Determine the theoretical yield of H₂S (in moles) if 32 mol Al₂S₃ and 32 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃= 150.17 g/mol. Al₂S₃(s) + 6 H₂O(l) → 2 Al(OH) ₃(s) + 3 H₂S(g)

The density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 30.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(l)

8.0 g of iron is reacted with 8.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE? 3 Fe(s) + 4 H₂O(l) → Fe₃O₄(s) + 4 H₂(g)

When 13.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s) + 2 H₂O(l) → Ca(OH) ₂(aq) + H₂(g)

10 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE? N₂(g) + 3 H₂(g) → 2 NH₃(g)

When 8.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced? 4 NH₃(g) + 3 O₂(g) → 2 N₂(g) + 6 H₂O(g)