Question 1

What is the concentration of FeCl₃ in a solution prepared by dissolving 20.0 g of FeCl₃ in enough water to make 275 mL of solution?

Accepted Answer

First, we need to convert the mass of FeCl₃ to moles using its molar mass. The molar mass of FeCl₃ is 162.2 g/mol (55.85 + 35.45 + 36.90). 20.0 g FeCl₃ x (1 mol FeCl₃ / 162.2 g FeCl₃) = 0.1231 mol FeCl₃ Next, we need to divide the moles of FeCl₃ by the volume of the solution in liters. 275 mL = 0.275 L Concentration = 0.1231 mol / 0.275 L = 0.448 mol/L Therefore, the answer is B) 0.448 mol/L.

Question 2

How many grams of AgNO₃ are needed to make 250.mL of a solution that is 0.135 mol L^-1?

Accepted Answer

To determine the amount of AgNO₃ needed, we can use the formula: moles = concentration x volume First, we need to convert the given volume from mL to L: 250.mL / 1000.mL/L = 0.250 L Then, we can substitute the given values into the formula: moles = 0.135 mol L^-1/L x 0.250 L = 0.03375 mol L^-1 To convert moles to grams, we can use the molar mass of AgNO₃: AgNO₃: Ag = 1 x 107.87 g/mol, N = 1 x 14.01 g/mol, O = 4 x 16.00 g/mol, S = 1 x 32.06 g/mol Molar mass = 107.87 g/mol + 14.01 g/mol + 4 x 16.00 g/mol + 32.06 g/mol = 265.94 g/mol grams = moles x molar mass = 0.03375 mol L^-1 x 265.94 g/mol ≈ 8.98 g Therefore, the best choice is C) 5.73 g.

Question 3

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? 2S(s)+ 3O₂(g)+ 4NaOH(aq)→ 2Na₂SO₄(aq)+ 2H₂O(l)

Accepted Answer

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

Question 4

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

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). The mass of sodium is given as 5.98 g, and the masses of hydrogen and sodium hydroxide produced are 0.26 g and 10.40 g, respectively. The total mass after the reaction is 0.26 g + 10.40 g = 10.66 g. To find the mass of water, subtract the mass of sodium from the total mass after the reaction: 10.66 g - 5.98 g = 4.68 g.

Question 5

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 16.8 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

Accepted Answer

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Question 6

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

1) Write the balanced chemical equation: AgNO3 + BaCl2 → AgCl + Ba(NO3)2
2) Find the limiting reactant: we need to find how many moles of each reactant we have, and then compare the mole ratio from the balanced equation.

- For silver nitrate: 10.0 g / 169.87 g/mol = 0.0589 mol
- For barium chloride: 15.0 g / 208.23 g/mol = 0.0721 mol

The mole ratio of AgNO3 : BaCl2 is 1:1, but we have more moles of BaCl2, so it is the limiting reactant.

3) Use stoichiometry to find the mass of AgCl:

- 0.0721 mol BaCl2 × 1 mol AgCl / 1 mol BaCl2 × 143.32 g/mol = 10.32 g AgCl

Therefore, the answer is A, 8.44 g, because we started with only 0.0589 mol AgNO3 so we cannot get more than that amount of AgCl.

Question 7

How many grams of H₃PO₄ are in 265 mL of a 1.50 mol L^-1 solution of H₃PO₄ ?

Accepted Answer

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Question 8

Calculate the number of grams of solute in 500.0 mL of 0.189 mol L^-1 KOH.

Accepted Answer

The answer of Calculate the number of grams of solute...

Question 9

What is the concentration (M)of sodium ions in 4.57 L of a 1.25 mol L^-1 $\mathrm { Na } _ { 3 }$ P solution?

Accepted Answer

The answer of What is the concentration (M)of sodium ions...

Question 10

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: 
CaO(s)+ $\mathrm { H } _ { 2 }$ O(l)? $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }$ (s)
In a particular experiment,5.00 g sample of CaO is reacted with excess water and 6.11 g of $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }$ is recovered.What is the percent yield in this experiment?

Accepted Answer

The balanced equation tells us that one mole of CaO reacts with one mole of water to produce one mole of Ca(OH)2. We can use the molar mass of Ca(OH)2 to convert the mass recovered to moles of Ca(OH)2 produced:

6.11 g Ca(OH)2 x (1 mol Ca(OH)2 / 74.09 g Ca(OH)2) = 0.0826 mol Ca(OH)2

Since one mole of CaO produces one mole of Ca(OH)2, we know that the theoretical yield of Ca(OH)2 is also 0.0826 mol. We can use the molar mass of CaO to convert the mass used to moles of CaO:

5.00 g CaO x (1 mol CaO / 56.08 g CaO) = 0.0891 mol CaO

The percent yield is then calculated as:

(actual yield / theoretical yield) x 100%
= (0.0826 mol / 0.0891 mol) x 100%
= 92.5%

Question 11

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)+ 3H₂(g)→ 2NH₃(g)

Accepted Answer

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

Question 12

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)+ 2H₂O(l)→ Ca(OH)₂(aq)+ H₂(g)

Accepted Answer

First, we need to calculate the theoretical yield of calcium hydroxide that should be produced based on the given amount of calcium metal used. 
Molar mass of Ca = 40.08 g/mol 
11.0 g of Ca = 11.0 g / 40.08 g/mol = 0.274 mol Ca 
From the balanced equation, 1 mole of Ca produces 1 mole of Ca(OH)2 
Therefore, 0.274 mol of Ca produces 0.274 mol of Ca(OH)2 
Molar mass of Ca(OH)2 = 74.09 g/mol 
0.274 mol of Ca(OH)2 = 20.3 g of Ca(OH)2 (theoretical yield)

Now, we can calculate the percent yield: 
Actual yield = 5.00 g 
Percent yield = (actual yield / theoretical yield) x 100% 
Percent yield = (5.00 g / 20.3 g) x 100% = 24.6%

The closest choice to our calculated percent yield is B, 24.6%.

Question 13

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? 3Fe(s)+ 4H₂O(l)→ Fe₃O₄(s)+ 4H₂(g)

Accepted Answer

In order to determine the limiting reactant, we need to calculate the amount of product that can be formed from both reactants. 
From the balanced equation, we can see that 3 moles of Fe reacts with 4 moles of H2O to produce 1 mole of FeS13O14 and 4 moles of H2. 
Using the given masses, we can calculate the moles of each reactant:
moles of Fe = 5.0 g / 55.85 g/mol = 0.089
moles of H2O = 5.0 g / 18.015 g/mol = 0.278
Now we can determine the amount of product that can be formed from each reactant:
Fe: 0.089 moles Fe x (1 mole FeS13O14 / 3 moles Fe) x (87.91 g/mol FeS13O14) = 2.66 g FeS13O14
H2O: 0.278 moles H2O x (1 mole FeS13O14 / 4 moles H2O) x (87.91 g/mol FeS13O14) = 6.81 g FeS13O14
Since Fe can only produce 2.66 g of FeS13O14, while H2O can produce 6.81 g, water is the limiting reactant. Therefore, statement D is false.

Question 14

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 15

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? 3NO₂(g)+ H₂O(l)→ 2HNO₃(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 16

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? 4NH₃(g)+ 3O₂(g)→ 2N₂(g)+ 6H₂O(g)

Accepted Answer

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Question 17

What volume of a 0.540 mol L^-1 NaOH solution contains 11.5 g of NaOH?

Accepted Answer

The answer of What volume of a 0.540 mol L^-1...

Question 18

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+ H₂O(l)? $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }$ (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 19

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ $\mathrm { N } _ { 2 }$ (g)? $2 \mathrm { Li } _ { 3 }$ N(s)
In a particular experiment,5.50 g samples of each reagent are reacted.What is the theoretical yield of lithium nitride?

Accepted Answer

The theoretical yield is calculated based on the limiting reagent. First, calculate moles of each reactant: Li: 5.50 g / 6.94 g/mol = 0.792 mol; N2: 5.50 g / 28.02 g/mol = 0.196 mol. The reaction requires 6 moles of Li for every 1 mole of N2, so Li is the limiting reagent. The moles of Li3N produced is 0.792 mol Li / 6 = 0.132 mol Li3N. The mass of Li3N is 0.132 mol * 34.83 g/mol = 4.60 g.

Question 20

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Accepted Answer

The answer of What is the concentration (M)of a NaCl...

Quiz 4: Chemical Reactions and Stoichiometry

What is the concentration of FeCl₃ in a solution prepared by dissolving 20.0 g of FeCl₃ in enough water to make 275 mL of solution?

How many grams of AgNO₃ are needed to make 250.mL of a solution that is 0.135 mol L^-1?

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? 2S(s) + 3O₂(g) + 4NaOH(aq) → 2Na₂SO₄(aq) + 2H₂O(l)

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?

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 16.8 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

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?

How many grams of H₃PO₄ are in 265 mL of a 1.50 mol L^-1 solution of H₃PO₄ ?

Calculate the number of grams of solute in 500.0 mL of 0.189 mol L^-1 KOH.

What is the concentration (M)of sodium ions in 4.57 L of a 1.25 mol L^-1 $\mathrm { Na } _ { 3 }$ P solution?

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) + 3H₂(g) → 2NH₃(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) + 2H₂O(l) → Ca(OH) ₂(aq) + H₂(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? 3Fe(s) + 4H₂O(l) → Fe₃O₄(s) + 4H₂(g)

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? 3NO₂(g) + H₂O(l) → 2HNO₃(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? 4NH₃(g) + 3O₂(g) → 2N₂(g) + 6H₂O(g)

What volume of a 0.540 mol L^-1 NaOH solution contains 11.5 g of NaOH?

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) ? $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }$ (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?

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + $\mathrm { N } _ { 2 }$ (g) ? $2 \mathrm { Li } _ { 3 }$ N(s) In a particular experiment,5.50 g samples of each reagent are reacted.What is the theoretical yield of lithium nitride?

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Quiz 4: Chemical Reactions and Stoichiometry

What is the concentration of FeCl3 in a solution prepared by dissolving 20.0 g of FeCl3 in enough water to make 275 mL of solution?

How many grams of AgNO3 are needed to make 250.mL of a solution that is 0.135 mol L-1?

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? 2S(s) + 3O2(g) + 4NaOH(aq) → 2Na2SO4(aq) + 2H2O(l)

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?

What is the concentration (M)of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?

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?

How many grams of H3PO4 are in 265 mL of a 1.50 mol L-1 solution of H3PO4 ?

Calculate the number of grams of solute in 500.0 mL of 0.189 mol L-1 KOH.

What is the concentration (M)of sodium ions in 4.57 L of a 1.25 mol L-1 Na3\mathrm { Na } _ { 3 }Na3​ P solution?

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) + 3H2(g) → 2NH3(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) + 2H2O(l) → Ca(OH) 2(aq) + H2(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? 3Fe(s) + 4H2O(l) → Fe3O4(s) + 4H2(g)

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? 3NO2(g) + H2O(l) → 2HNO3(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? 4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g)

What volume of a 0.540 mol L-1 NaOH solution contains 11.5 g of NaOH?

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) ? Ca(OH) 2\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }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?

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2\mathrm { N } _ { 2 }N2​ (g) ? 2Li32 \mathrm { Li } _ { 3 }2Li3​ N(s) In a particular experiment,5.50 g samples of each reagent are reacted.What is the theoretical yield of lithium nitride?

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

What is the concentration of FeCl₃ in a solution prepared by dissolving 20.0 g of FeCl₃ in enough water to make 275 mL of solution?

How many grams of AgNO₃ are needed to make 250.mL of a solution that is 0.135 mol L^-1?

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? 2S(s) + 3O₂(g) + 4NaOH(aq) → 2Na₂SO₄(aq) + 2H₂O(l)

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 16.8 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

How many grams of H₃PO₄ are in 265 mL of a 1.50 mol L^-1 solution of H₃PO₄ ?

Calculate the number of grams of solute in 500.0 mL of 0.189 mol L^-1 KOH.

What is the concentration (M)of sodium ions in 4.57 L of a 1.25 mol L^-1 $\mathrm { Na } _ { 3 }$ P solution?

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) + 3H₂(g) → 2NH₃(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) + 2H₂O(l) → Ca(OH) ₂(aq) + H₂(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? 3Fe(s) + 4H₂O(l) → Fe₃O₄(s) + 4H₂(g)

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? 3NO₂(g) + H₂O(l) → 2HNO₃(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? 4NH₃(g) + 3O₂(g) → 2N₂(g) + 6H₂O(g)

What volume of a 0.540 mol L^-1 NaOH solution contains 11.5 g of NaOH?

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H₂O(l) ? $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }$ (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?

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + $\mathrm { N } _ { 2 }$ (g) ? $2 \mathrm { Li } _ { 3 }$ N(s) In a particular experiment,5.50 g samples of each reagent are reacted.What is the theoretical yield of lithium nitride?