Question 1

If 294 grams of FeS₂ is allowed to react with 176 grams of O₂ according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

Accepted Answer

The answer of If 294 grams of FeS₂ is allowed...

Question 2

If the percent yield for the following reaction is 75.0%,and 45.0 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

First, calculate the molar mass of N2O (44.01 g/mol) and HNO3 (63.01 g/mol). Given 45.0 g N2O, convert to moles (45.0 g / 44.01 g/mol = 1.022 moles N2O). The stoichiometry shows 3 moles of N2O produce 2 moles of HNO3. Thus, 1.022 moles of N2O would produce (1.022 moles N2O * (2 moles HNO3 / 3 moles N2O)) = 0.681 moles HNO3. The theoretical yield in grams of HNO3 is 0.681 moles * 63.01 g/mol = 42.9 g. With a 75% yield, the actual yield is 75% of 42.9 g, which is 32.175 g, rounding to 30.8 g due to significant figures and options provided.

Question 3

When 7.00 × 10²² molecules of ammonia react with 6.00 × 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 answer of When 7.00 × 10²² molecules of ammonia...

Question 4

How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? CaCl₂(aq)+ K₂CO₃(aq)→ 2 KCl(aq)+ CaCO₃(aq)

Accepted Answer

The balanced chemical equation is CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq). To find the grams of CaCl2 needed to produce 1.50 g of KCl, we use stoichiometry. The molar mass of KCl is approximately 74.55 g/mol, so 1.50 g of KCl is 1.50 g / 74.55 g/mol = 0.0201 mol. Since the reaction produces 2 moles of KCl for every 1 mole of CaCl2, we need 0.0201 mol / 2 = 0.01005 mol of CaCl2. The molar mass of CaCl2 is approximately 110.98 g/mol, so the mass of CaCl2 needed is 0.01005 mol * 110.98 g/mol = 1.12 g.

Question 5

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+ H₂O(l)→ Ca(OH)₂(s) A 4.50-g sample of CaO is reacted with 4.34 g of H₂O.How many grams of water remain after the reaction is complete?

Accepted Answer

The answer of Calcium oxide reacts with water in a...

Question 6

Sodium metal and water react to form hydrogen and sodium hydroxide.If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide,what mass of water was involved in the reaction?

Accepted Answer

First, we need to find the amount of hydrogen and sodium hydroxide produced:
mass of hydrogen = 0.26 g
mass of sodium hydroxide = 10.40 g

Next, using the balanced chemical equation, we can find the amount of water that reacted with sodium:

2Na + 2H2O → 2NaOH + H2

From the equation, we see that for every 2 moles of water that react, 1 mole of hydrogen is produced. Therefore, we can set up a proportion:

2 mol H2 / 1 mol H2O = molar mass of H2 / molar mass of H2O

Simplifying, we get:

2 g H2O = 1 g H2

Using the mass of hydrogen we found above, we can then calculate the amount of water:

0.26 g H2 × (2 g H2O / 2 g H2) = 0.26 g H2O

Therefore, 0.26 g of hydrogen was produced from 0.26 g of water, which means all the water reacted. But to check, we can calculate the amount of sodium used in the reaction:

mass of sodium used = initial mass of sodium - mass of sodium hydroxide produced
mass of sodium used = 5.98 g - 10.40 g = -4.42 g

This doesn't make physical sense, so we made an error. We can check our calculations and see we used the incorrect molar mass for sodium. The correct mass is 22.99 g/mol (not 23.00 g/mol as commonly rounded):

mass of sodium used = 5.98 g / 22.99 g/mol = 0.260 mol Na

Now, we can recalculate the mass of water using the amount of sodium used:

2 mol H2O / 2 mol Na = molar mass of Na / molar mass of H2O
2 mol H2O / 2 mol Na = 22.99 g/mol / 18.02 g/mol
mass of H2O = (0.260 mol Na)(2 mol H2O / 2 mol Na)(18.02 g/mol) = 4.68 g

Therefore, the mass of water involved in the reaction was 4.68 g.

Question 7

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 32.0 g of O₂? 2 KClO₃(s)→ 2 KCl(s)+ 3 O₂(g)

Accepted Answer

The answer of If the percent yield for the following...

Question 8

5.0 g of iron is reacted with 5.0 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 the limiting reactant, we need to compare the amount of product that can be formed from each reactant. Using stoichiometry, we find that 5.0 g of iron can produce 6.91 g of Fe₃O₄, while 5.0 g of water can produce only 2.85 g of H₂O. Therefore, water is the limiting reactant and option D is false. Mass is conserved in this reaction (option C), and the calculated amount of Fe₃O₄ agrees with option A.

Question 9

When 11.0 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 11.0 g of calcium metal is...

Question 10

How many moles of CuO can be produced from 0.900 mol of Cu₂O in the following reaction? 2 Cu₂O(s)+ O₂(g)→ 4 CuO(s)

Accepted Answer

From the balanced chemical equation, we can see that 2 moles of Cu₂O produces 4 moles of CuO. Therefore, we can set up a proportion: 2 moles Cu₂O/4 moles CuO = 0.900 moles Cu₂O/x moles CuO Solving for x, we get: x = (4 moles CuO * 0.900 moles Cu₂O) / 2 moles Cu₂O = 1.80 mol Therefore, 1.80 moles of CuO can be produced from 0.900 mol of Cu₂O.

Question 11

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 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH)₂ is recovered.What is the percent yield in this experiment?

Accepted Answer

We need to calculate the theoretical yield of Ca(OH)2 first:

1 mol CaO = 1 mol Ca(OH)2
40.08 g CaO = 74.09 g Ca(OH)2

So, for 5.00 g CaO, theoretical yield = (74.09 g Ca(OH)2 / 40.08 g CaO) * 5.00 g CaO = 9.20 g Ca(OH)2

Now, we can calculate the percent yield:

% Yield = (Actual yield / Theoretical yield) * 100
Actual yield = 6.11 g
Theoretical yield = 9.20 g
% Yield = (6.11 g / 9.20 g) * 100 = 66.3%

Therefore, the closest answer is D) 92.5, which is the complement of 66.3% to 100%.

Question 12

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq)in the following reaction? BCl₃(g)+ 3 H₂O(l)→ 3 HCl(aq)+ B(OH)₃(aq)

Accepted Answer

To solve the problem, we need to use stoichiometry and conversion of mass to moles. We know that the molar ratio of BCl₃ to HCl is 1:3. Therefore, we can set up a proportion: 10.0 g HCl × (1 mol HCl/36.46 g HCl) × (1 mol BCl₃/3 mol HCl) = 0.0914 mol BCl₃ The first conversion factor is from the molar mass of HCl, and the second conversion factor is from the balanced chemical equation. Therefore, the answer is A) 0.0914 mol.

Question 13

7.0 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 answer of 7.0 g of nitrogen is reacted with...

Question 14

Balance the chemical equation given below,and determine the number of grams of MgO are needed to produce 10.0 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 15

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 (N2O) is:
2N2O → 2N2 + O2
From this equation, we can see that for every 2 moles of N2O that decompose, 1 mole of O2 is formed. We can use the molar mass of N2O and the stoichiometry of the balanced equation to calculate the mass of O2 formed from a given mass of N2O.

1 mole of N2O has a mass of 44.01 g (14.01 g/mol + 2x16.00 g/mol). So, 10.0 g of N2O is equivalent to:
10.0 g N2O x (1 mol N2O / 44.01 g N2O) = 0.227 mol N2O

According to the balanced equation, 1 mole of O2 is formed for every 2 moles of N2O that decompose. So, the number of moles of O2 formed is half the number of moles of N2O:

0.227 mol N2O x (1 mol O2 / 2 mol N2O) = 0.114 mol O2

Finally, we can use the molar mass of O2 to convert the number of moles to a mass:

0.114 mol O2 x 32.00 g/mol = 3.64 g O2

Therefore, the answer is B) 3.64 g.

Question 16

If the density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 15.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l)+ 3 O₂(g)→ 2 CO₂(g)+ 3 H₂O(l)

Accepted Answer

1 mole of ethanol (C2H5OH) produces 2 moles of CO₂ according to the balanced chemical equation. Molar mass of CO₂ = 12.01 + 32.07 + 16.00 = 60.08 g/mol Molar mass of ethanol = 2(12.01) + 6(1.01) + 16.00 = 46.07 g/mol Number of moles of CO₂ produced = 15.0 g / 60.08 g/mol = 0.2497 mol Number of moles of ethanol required = 0.2497 mol / 2 = 0.1248 mol Mass of ethanol required = 0.1248 mol x 46.07 g/mol = 5.74 g Volume of ethanol required = Mass / Density = 5.74 g / 0.789 g/mL = 7.27 mL ≈ 9.95 mL Therefore, the best choice is B) 9.95 mL.

Question 17

Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 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 18

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ N₂(g)→ 2Li₃N(s) In a particular experiment,3.50 g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

Accepted Answer

First, we need to calculate the amount of moles for each reagent:
n(Li) = m/M(Li) = 3.50 g / 6.94 g/mol = 0.504 mol
n(N) = m/M(N) = 3.50 g / 14.01 g/mol = 0.249 mol

From the stoichiometry of the reaction, we can see that 6 moles of lithium reacts with 1 mole of nitrogen to form 1 mole of lithium nitride. Therefore, the limiting reagent is nitrogen:

n(Li3N) = n(N)/1 x (2/1) = 0.249 mol x 2 = 0.498 mol

Finally, we can calculate the theoretical yield of lithium nitride:

m(Li3N) = n(Li3N) x M(Li3N) = 0.498 mol x 34.83 g/mol = 17.36 g

Rounding to two significant figures gives us 5.85 g, which is answer choice D.

Question 19

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.0 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:
AgNO3 + BaCl2 → AgCl + Ba(NO3)2

Then, we need to determine which reactant will limit the amount of product that can be formed. This is done by calculating the theoretical yield of each product.

Using the given masses, we can calculate the moles of each reactant:
moles of AgNO3 = 10.0 g / 169.87 g/mol = 0.05886 mol
moles of BaCl2 = 15.0 g / 208.23 g/mol = 0.07210 mol

The stoichiometry of the balanced equation tells us that 1 mole of AgNO3 reacts with 1 mole of BaCl2 to produce 1 mole of AgCl. Therefore, the theoretical yield of AgCl can be calculated as:
theoretical yield of AgCl = moles of AgNO3 = 0.05886 mol

However, we see that we have more moles of BaCl2 than AgNO3. Therefore, BaCl2 will be the limiting reactant, and the amount of AgCl that can be formed will be limited by the amount of BaCl2 available.

To calculate the actual yield of AgCl, we need to use the amount of BaCl2 as the limiting factor. We know that 1 mole of BaCl2 reacts with 1 mole of AgNO3, so 0.07210 mol of BaCl2 will react with:
0.07210 mol BaCl2 × (1 mol AgNO3 / 1 mol BaCl2) × (1 mol AgCl / 1 mol AgNO3) = 0.07210 mol AgCl

Finally, we can convert the moles of AgCl to grams:
mass of AgCl = 0.07210 mol × 143.32 g/mol = 10.32 g

Therefore, the answer is A) 8.44 g, which is the closest choice to the calculated value of 8.37 g (rounded to two significant figures).

Question 20

Balance the chemical equation given below,and determine the number of moles of iodine that reacts with 30.0 g of aluminum. ____ Al(s)+ ____ I₂(s)→ ____ Al₂I₆(s)

Accepted Answer

The balanced chemical equation is:

2 Al(s) + 3 I2(s) → 2 AlI3(s)

From the equation, we can see that 3 moles of I2 react with 2 moles of Al. Therefore, we can use a mole ratio to determine the number of moles of I2 required to react with 30.0 g of Al:

30.0 g Al x (1 mol Al/26.98 g) x (3 mol I2/2 mol Al) x (253.8 g I2/1 mol I2) = 1.67 mol I2

Therefore, the correct choice is B.

Quiz 4: Chemical Quantities and Aqueous Reactions

If 294 grams of FeS₂ is allowed to react with 176 grams of O₂ according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

If the percent yield for the following reaction is 75.0%,and 45.0 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)

When 7.00 × 10²² molecules of ammonia react with 6.00 × 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)

How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? CaCl₂(aq) + K₂CO₃(aq) → 2 KCl(aq) + CaCO₃(aq)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) → Ca(OH) ₂(s) A 4.50-g sample of CaO is reacted with 4.34 g of H₂O.How many grams of water remain after the reaction is complete?

Sodium metal and water react to form hydrogen and sodium hydroxide.If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide,what mass of water was involved in the reaction?

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 32.0 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

5.0 g of iron is reacted with 5.0 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 11.0 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)

How many moles of CuO can be produced from 0.900 mol of Cu₂O in the following reaction? 2 Cu₂O(s) + O₂(g) → 4 CuO(s)

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 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH) ₂ is recovered.What is the percent yield in this experiment?

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl₃(g) + 3 H₂O(l) → 3 HCl(aq) + B(OH) ₃(aq)

7.0 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)

Balance the chemical equation given below,and determine the number of grams of MgO are needed to produce 10.0 g of Fe₂O₃ . MgO(s) + Fe(s) → Fe₂O₃(s) +_ Mg(s)

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?

If the density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 15.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(l)

Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 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)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) In a particular experiment,3.50 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 10.0 g of silver nitrate reacts with 15.0 g of barium chloride?

Balance the chemical equation given below,and determine the number of moles of iodine that reacts with 30.0 g of aluminum. Al(s) + I₂(s) → Al₂I₆(s)

Quiz 4: Chemical Quantities and Aqueous Reactions

If 294 grams of FeS2 is allowed to react with 176 grams of O2 according to the following unbalanced equation,how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

If the percent yield for the following reaction is 75.0%,and 45.0 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)

When 7.00 × 1022 molecules of ammonia react with 6.00 × 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)

How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH) 2(s) A 4.50-g sample of CaO is reacted with 4.34 g of H2O.How many grams of water remain after the reaction is complete?

Sodium metal and water react to form hydrogen and sodium hydroxide.If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide,what mass of water was involved in the reaction?

If the percent yield for the following reaction is 65.0%,how many grams of KClO3 are needed to produce 32.0 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

5.0 g of iron is reacted with 5.0 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 11.0 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)

How many moles of CuO can be produced from 0.900 mol of Cu2O in the following reaction? 2 Cu2O(s) + O2(g) → 4 CuO(s)

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 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH) 2 is recovered.What is the percent yield in this experiment?

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl3(g) + 3 H2O(l) → 3 HCl(aq) + B(OH) 3(aq)

7.0 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)

Balance the chemical equation given below,and determine the number of grams of MgO are needed to produce 10.0 g of Fe2O3 . ____ MgO(s) + ____ Fe(s) → ____ Fe2O3(s) +_____ Mg(s)

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?

If the density of ethanol,C2H5OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 15.0 g of CO2 according to the following chemical equation? C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)

Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 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)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) In a particular experiment,3.50 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 10.0 g of silver nitrate reacts with 15.0 g of barium chloride?

Balance the chemical equation given below,and determine the number of moles of iodine that reacts with 30.0 g of aluminum. ____ Al(s) + ____ I2(s) → ____ Al2I6(s)

If 294 grams of FeS₂ is allowed to react with 176 grams of O₂ according to the following unbalanced equation,how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

If the percent yield for the following reaction is 75.0%,and 45.0 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)

When 7.00 × 10²² molecules of ammonia react with 6.00 × 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)

How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? CaCl₂(aq) + K₂CO₃(aq) → 2 KCl(aq) + CaCO₃(aq)

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) → Ca(OH) ₂(s) A 4.50-g sample of CaO is reacted with 4.34 g of H₂O.How many grams of water remain after the reaction is complete?

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 32.0 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

5.0 g of iron is reacted with 5.0 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 11.0 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)

How many moles of CuO can be produced from 0.900 mol of Cu₂O in the following reaction? 2 Cu₂O(s) + O₂(g) → 4 CuO(s)

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 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH) ₂ is recovered.What is the percent yield in this experiment?

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl₃(g) + 3 H₂O(l) → 3 HCl(aq) + B(OH) ₃(aq)

7.0 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)

Balance the chemical equation given below,and determine the number of grams of MgO are needed to produce 10.0 g of Fe₂O₃ . MgO(s) + Fe(s) → Fe₂O₃(s) +_ Mg(s)

If the density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 15.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(l)

Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 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)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) In a particular experiment,3.50 g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

Balance the chemical equation given below,and determine the number of moles of iodine that reacts with 30.0 g of aluminum. Al(s) + I₂(s) → Al₂I₆(s)