Question 1

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3H₂O → ICl + HIO₃ + 5HCl

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Question 2

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows: H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g)+ H₂O(l)→ 2HNO₃(aq)+ NO(g)

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Question 3

According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2H₂S(g)+ SO₂(g)→ 3S(s)+ 2H₂O(l)

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Question 4

How many moles of nitrogen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s)→ 2K₂O(s)+ 2N₂(g)+ 5O₂(g)

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Question 5

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s)→ 2K₂O(s)+ 2N₂(g)+ 5O₂(g)

Accepted Answer

1 mol of KNO₃ produces 5 mol of O₂ Therefore, 58.6 g of KNO₃ is equal to (58.6/101.11) = 0.579 mol of KNO₃ Using stoichiometry of the reaction, 4 KNO₃ → 5 O₂ 0.579 mol → (5/4) x 0.579 mol = 0.724 mol of O₂. Therefore, the answer is D.

Question 6

Give the theoretical yield, in moles, of CO₂from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂. 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

Accepted Answer

From the balanced equation, we can see that the mole ratio between C₈H₁₈ and CO₂ is 2:16 or 1:8. Therefore, the theoretical yield of CO₂ will be 8 times the amount of C₈H₁₈ used. Since 4.00 moles of C₈H₁₈ are used, the theoretical yield of CO₂ will be: 8 x 4.00 moles = 32.00 moles However, we need to check if there is enough O₂ to fully react with all of the C₈H₁₈. The ratio between C₈H₁₈ and O₂ is 2:25, so we need 25/2 = 12.5 moles of O₂ to react with 4.00 moles of C₈H₁₈. Since we only have 4.00 moles of O₂, it is the limiting reagent and will be fully consumed in the reaction. Therefore, the theoretical yield of CO₂ is: 4.00 moles x (16/25) = 2.56 moles Thus, the best choice is C.

Question 7

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s)+ 2H₂O(l)→ 4KOH(s)+ O₂(g)

Accepted Answer

From the balanced equation, we can see that 2 moles of H₂O react with 4 moles of KOH. This means that 1 mole of H₂O will react with 4/2 = 2 moles of KOH. Therefore, 5.44 moles of H₂O will react with 5.44 x 2/2 = 10.9 moles of KOH. Since there is an excess of KOH, all of the 10.9 moles of KOH will be formed.

Question 8

How many grams of Li₃N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6Li(s)+ N₂(g)→ 2Li₃N(s)

Accepted Answer

Using the mole ratio from the balanced equation, we see that for every 6 moles of Li that react, we get 2 moles of Li₃N formed. Therefore, for 1.75 moles of Li, we can expect (1.75 mol Li) x (2 mol Li₃N / 6 mol Li) = 0.58 moles Li₃N to be formed. To convert the moles of Li₃N to grams, we need to use its molar mass. Li: 6.94 g/mol S: 32.07 g/mol N: 14.01 g/mol B: 10.81 g/mol Molar mass of Li₃N: (3 x Li) + S + (2 x B) + N = (3 x 6.94) + 32.07 + (2 x 10.81) + 14.01 = 58.69 g/mol Now, we can calculate the mass of Li₃N: (0.58 mol Li₃N) x (58.69 g Li₃N / 1 mol Li₃N) = 34.12 g Li₃N Therefore, the answer is B: 20.3 g Li₃N (rounded to two significant figures).

Question 9

Determine the limiting reactant (LR)and the mass (in g)of nitrogen that can be formed from 50.0 g N₂O₄ and 45.0 g N₂H₄. Some possibly useful molar masses are as follows: N₂O₄ = 92.02 g mol^-1, N₂H₄ = 32.05 g mol^-1. N₂O₄(l)+ 2N₂H₄(l)→ 3N₂(g)+ 4H₂O(g)

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Question 10

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H₂O? 4KO(s)+ 2H₂O(l)→ 4KOH(s)+ O₂(g)

Accepted Answer

From the balanced reaction, we see that 4 moles of KO react with 2 moles of H₂O. Therefore, we can set up a proportion: 4 moles KO/2 moles H₂O = x moles KO/5.44 moles H₂O Solving for x, we get: x = (4/2) * 5.44 = 10.88 Rounding to two decimal places, we get 10.9 moles KO as the answer.

Question 11

Determine the theoretical yield of H₂S (in moles)if 4.0 mol Al₂S₃ and 4.0 mol H₂O are reacted according to the following balanced reaction. A possibly useful molar mass is Al₂S₃= 150.17 g mol^-1. Al₂S₃(s)+ 6H₂O(l)→ 2Al(OH)₃(s)+ 3H₂S(g)

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Question 12

Consider the following balanced reaction. What mass (in g)of CO₂ can be formed from 288 mg of O₂? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6O₂(g)→ 3CO₂(g)+ SO₂(g)+ 4H₂O(g)

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Question 13

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kilograms of iodine were produced?

Accepted Answer

The correct answer is C) 79.4 kg.Explanation:The ratio of potassium to iodine in potassium iodide is 1:1 by mass. Therefore, if the second sample produced 24.4 kg of potassium, it must have also produced 24.4 kg of iodine.

Question 14

A 14.01 g sample of N₂ reacts with 3.02 g of H₂ to form ammonia (NH₃). If ammonia is the only product, what mass of ammonia is formed?

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Question 15

How many molecules of H₂S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO₂. 2H₂S(g)+ SO₂(g)→ 3S(s)+ 2H₂O(l)

Accepted Answer

First, we need to find the moles of sulfur using its molar mass: $$79.0 ext{ g S} imes \frac{1 ext{ mol S}}{32.066 ext{ g S}} = 2.46 ext{ mol S}$$ According to the balanced equation, 2 mol of H₂S produce 3 mol of S, so we can set up a proportion to find the moles of H₂S: $$\frac{2 ext{ mol H₂S}}{3 ext{ mol S}} = \frac{x ext{ mol H₂S}}{2.46 ext{ mol S}}$$ Solving for x, we get: $$x = \frac{2.46 ext{ mol S} imes 2 ext{ mol H₂S}}{3 ext{ mol S}} = 1.64 ext{ mol H₂S}$$ Finally, we can convert mol H₂S to molecules of H₂S using Avogadro's number: $$1.64 ext{ mol H₂S} imes 6.022 imes 10^{23} ext{ molecules/mol} = 9.89 imes 10^{23} ext{ molecules of H₂S}$$ Therefore, the answer is choice B.

Question 16

Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H₂CO₃ → H₂O + CO₂

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Question 17

Two samples of calcium fluoride are decomposed into their constituent elements. The first sample produced 0.154 g of calcium and 0.146 g of fluorine. If the second sample produced 294 mg of fluorine, how many grams of calcium were formed?

Accepted Answer

The ratio of calcium to fluorine in the first sample is 0.154 g Ca / 0.146 g F. Using this ratio, for 294 mg (0.294 g) of fluorine in the second sample, the amount of calcium is (0.154/0.146) * 0.294 g = 0.309 g.

Question 18

How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4KO(s)+ 2H₂O(l)→ 4KOH(s)+ O₂(g)

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Question 19

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6O₂(g)→ 3CO₂(g)+ SO₂(g)+ 4H₂O (g)

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Question 20

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃). If it is the only product, what mass of PCl₃ is formed?

Accepted Answer

The balanced chemical equation for the reaction is:
P4 + 6Cl2 → 4PCl3
The molar mass of P4 is 123.9 g/mol and the molar mass of Cl2 is 70.9 g/mol. Using the coefficients from the balanced equation, we can calculate the amount of PCl3 that is formed:
(12.39 g P4) / (123.9 g/mol P4) x (4 mol PCl3 / 1 mol P4) x (137.33 g/mol PCl3) = 54.93 g PCl3
Therefore, the answer is choice B, 54.93 g.

Quiz 4: Chemical Reactions and Stoichiometry

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3H₂O → ICl + HIO₃ + 5HCl

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows: H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2H₂S(g) + SO₂(g) → 3S(s) + 2H₂O(l)

How many moles of nitrogen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s) → 2K₂O(s) + 2N₂(g) + 5O₂(g)

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s) → 2K₂O(s) + 2N₂(g) + 5O₂(g)

Give the theoretical yield, in moles, of CO₂from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂. 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

How many grams of Li₃N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6Li(s) + N₂(g) → 2Li₃N(s)

Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N₂O₄ and 45.0 g N₂H₄. Some possibly useful molar masses are as follows: N₂O₄ = 92.02 g mol^-1, N₂H₄ = 32.05 g mol^-1. N₂O₄(l) + 2N₂H₄(l) → 3N₂(g) + 4H₂O(g)

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H₂O? 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

Determine the theoretical yield of H₂S (in moles) if 4.0 mol Al₂S₃ and 4.0 mol H₂O are reacted according to the following balanced reaction. A possibly useful molar mass is Al₂S₃= 150.17 g mol^-1. Al₂S₃(s) + 6H₂O(l) → 2Al(OH) ₃(s) + 3H₂S(g)

Consider the following balanced reaction. What mass (in g) of CO₂ can be formed from 288 mg of O₂? Assume that there is excess C₃H₇SH present. C₃H₇SH(l) + 6O₂(g) → 3CO₂(g) + SO₂(g) + 4H₂O(g)

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kilograms of iodine were produced?

A 14.01 g sample of N₂ reacts with 3.02 g of H₂ to form ammonia (NH₃) . If ammonia is the only product, what mass of ammonia is formed?

How many molecules of H₂S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO₂. 2H₂S(g) + SO₂(g) → 3S(s) + 2H₂O(l)

Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H₂CO₃ → H₂O + CO₂

Two samples of calcium fluoride are decomposed into their constituent elements. The first sample produced 0.154 g of calcium and 0.146 g of fluorine. If the second sample produced 294 mg of fluorine, how many grams of calcium were formed?

How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C₃H₇SH present. C₃H₇SH(l) + 6O₂(g) → 3CO₂(g) + SO₂(g) + 4H₂O (g)

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃) . If it is the only product, what mass of PCl₃ is formed?

Quiz 4: Chemical Reactions and Stoichiometry

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3H2O → ICl + HIO3 + 5HCl

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g mol-1, HNO3 = 63.02 g mol-1. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)

According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2H2S(g) + SO2(g) → 3S(s) + 2H2O(l)

How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g mol-1. 4KNO3(s) → 2K2O(s) + 2N2(g) + 5O2(g)

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g mol-1. 4KNO3(s) → 2K2O(s) + 2N2(g) + 5O2(g)

Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2C8H18 + 25O2 → 16CO2 + 18H2O

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H2O? Assume an excess of KO. 4KO(s) + 2H2O(l) → 4KOH(s) + O2(g)

How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6Li(s) + N2(g) → 2Li3N(s)

Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g mol-1, N2H4 = 32.05 g mol-1. N2O4(l) + 2N2H4(l) → 3N2(g) + 4H2O(g)

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4KO(s) + 2H2O(l) → 4KOH(s) + O2(g)

Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g mol-1. Al2S3(s) + 6H2O(l) → 2Al(OH) 3(s) + 3H2S(g)

Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present. C3H7SH(l) + 6O2(g) → 3CO2(g) + SO2(g) + 4H2O(g)

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kilograms of iodine were produced?

A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3) . If ammonia is the only product, what mass of ammonia is formed?

How many molecules of H2S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO2. 2H2S(g) + SO2(g) → 3S(s) + 2H2O(l)

Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H2CO3 → H2O + CO2

Two samples of calcium fluoride are decomposed into their constituent elements. The first sample produced 0.154 g of calcium and 0.146 g of fluorine. If the second sample produced 294 mg of fluorine, how many grams of calcium were formed?

How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4KO(s) + 2H2O(l) → 4KOH(s) + O2(g)

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6O2(g) → 3CO2(g) + SO2(g) + 4H2O (g)

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3) . If it is the only product, what mass of PCl3 is formed?

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3H₂O → ICl + HIO₃ + 5HCl

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows: H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2H₂S(g) + SO₂(g) → 3S(s) + 2H₂O(l)

How many moles of nitrogen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s) → 2K₂O(s) + 2N₂(g) + 5O₂(g)

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s) → 2K₂O(s) + 2N₂(g) + 5O₂(g)

Give the theoretical yield, in moles, of CO₂from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂. 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

How many grams of Li₃N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6Li(s) + N₂(g) → 2Li₃N(s)

Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N₂O₄ and 45.0 g N₂H₄. Some possibly useful molar masses are as follows: N₂O₄ = 92.02 g mol^-1, N₂H₄ = 32.05 g mol^-1. N₂O₄(l) + 2N₂H₄(l) → 3N₂(g) + 4H₂O(g)

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H₂O? 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

Determine the theoretical yield of H₂S (in moles) if 4.0 mol Al₂S₃ and 4.0 mol H₂O are reacted according to the following balanced reaction. A possibly useful molar mass is Al₂S₃= 150.17 g mol^-1. Al₂S₃(s) + 6H₂O(l) → 2Al(OH) ₃(s) + 3H₂S(g)

Consider the following balanced reaction. What mass (in g) of CO₂ can be formed from 288 mg of O₂? Assume that there is excess C₃H₇SH present. C₃H₇SH(l) + 6O₂(g) → 3CO₂(g) + SO₂(g) + 4H₂O(g)

A 14.01 g sample of N₂ reacts with 3.02 g of H₂ to form ammonia (NH₃) . If ammonia is the only product, what mass of ammonia is formed?

How many molecules of H₂S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO₂. 2H₂S(g) + SO₂(g) → 3S(s) + 2H₂O(l)

Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H₂CO₃ → H₂O + CO₂

How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C₃H₇SH present. C₃H₇SH(l) + 6O₂(g) → 3CO₂(g) + SO₂(g) + 4H₂O (g)

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃) . If it is the only product, what mass of PCl₃ is formed?