Question 1

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

Water is not the limiting reactant. Iron is the limiting reactant because it is completely consumed in the reaction.

Question 2

When 5.00 × 10²² molecules of ammonia react with 4.00 × 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 5.00 × 10²² molecules of ammonia...

Question 3

Balance the chemical equation given below,and determine the number of grams of MgO needed to produce 15.0 g of Fe₂O₃. _____ MgO(s)+ _____ Fe(s)→ _____ Fe₂O₃(s)+ _____ Mg(s)

Accepted Answer

The balanced equation is 3MgO + 2Fe → Fe2O3 + 3Mg. The molar mass of Fe2O3 is 159.7 g/mol, and the molar mass of MgO is 40.3 g/mol. To produce 15.0 g of Fe2O3, you need (15.0 g / 159.7 g/mol) = 0.0939 mol of Fe2O3. From the balanced equation, 3 moles of MgO are needed for 1 mole of Fe2O3, so you need 0.0939 mol × 3 = 0.2817 mol of MgO. Therefore, you need 0.2817 mol × 40.3 g/mol = 11.4 g of MgO.

Question 4

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 5

How many grams of the excess reagent are left over when 6.00 g of CS₂ gas react with 10.0 g of Cl₂ gas in the following reaction: CS₂(g)+ 3 Cl₂(g)→ CCl₄(l)+ S₂Cl₂(l)

Accepted Answer

The answer of How many grams of the excess reagent...

Question 6

When methane,CH₄,undergoes combustion with oxygen,the usual products are carbon dioxide and water.Carbon monoxide is formed when the limiting reactant is

Accepted Answer

Carbon monoxide is typically formed during the incomplete combustion of methane, which occurs when there is not enough oxygen to produce carbon dioxide and water.

Question 7

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

The balanced chemical equation for the reaction between silver nitrate and barium chloride is:

AgNO3 + BaCl2 -> AgCl + Ba(NO3)2

To determine the amount of silver chloride formed, we first need to identify the limiting reactant. This can be done by calculating the amount of each reactant needed to completely react with each other based on their stoichiometric ratio.

From the balanced equation, we can see that:

1 mole of AgNO3 reacts with 1 mole of BaCl2 to produce 1 mole of AgCl

The molar masses of each compound are:

AgNO3 = 169.9 g/mol
BaCl2 = 208.3 g/mol

Using these values, we can calculate the number of moles of each reactant:

Number of moles of AgNO3 = 10.0 g / 169.9 g/mol = 0.05886 mol
Number of moles of BaCl2 = 15.0 g / 208.3 g/mol = 0.07202 mol

Based on the stoichiometric ratio, we can see that AgNO3 is the limiting reactant since it produces less moles of AgCl compared to BaCl2. Therefore, we will use the amount of AgNO3 to calculate the amount of AgCl formed.

Number of moles of AgCl = 0.05886 mol

The molar mass of AgCl is:

AgCl = 143.3 g/mol

Using this value, we can calculate the mass of AgCl formed:

Mass of AgCl = Number of moles of AgCl x Molar mass of AgCl
Mass of AgCl = 0.05886 mol x 143.3 g/mol
Mass of AgCl = 8.44 g

Therefore, the answer is (A) 8.44 g.

Question 8

When iron(III)oxide reacts with hydrochloric acid,iron(III)chloride and water are formed.How many grams of iron(III)chloride are formed from 10.0 g of iron(III)oxide and 10.0 g of hydrochloric acid?

Accepted Answer

First, we need to write the balanced chemical equation:
Fe2O3 + 6HCl → 2FeCl3 + 3H2O

Next, we need to determine the limiting reagent. To do this, we can use the mole ratio between iron(III)oxide and hydrochloric acid:

Fe2O3: 1 mole Fe2O3 = 2 moles FeCl3 (from balanced equation)
HCl: 6 moles HCl = 2 moles FeCl3 (from balanced equation)

Based on these ratios, we can see that 1 mole of Fe2O3 will react with 6/2 = 3 moles of HCl to produce 2 moles of FeCl3.

Now we can calculate the moles of each substance given in the problem:

moles Fe2O3 = 10.0 g / 159.69 g/mol = 0.0626 mol
moles HCl = 10.0 g / 36.46 g/mol = 0.274 mol

Since Fe2O3 is the limiting reagent (it produces less moles of product), we can use its mole ratio with FeCl3 to calculate the moles of FeCl3 produced:

moles FeCl3 = 2/1 x 0.0626 mol = 0.1253 mol

Finally, we can convert moles of FeCl3 to grams:

grams FeCl3 = 0.1253 mol x 162.2 g/mol = 20.3 g

Therefore, the answer is B) 14.8 g.

Question 9

Molarity is defined as

Accepted Answer

Molarity is defined as the number of moles of solute dissolved per liter of solution. It is independent of the amount or type of solvent present in the solution.

Question 10

When 10.0 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 theoretical yield of calcium hydroxide is calculated using stoichiometry. The molar mass of calcium is 40.08 g/mol, so 10.0 g of calcium is 0.249 mol. According to the balanced equation, 1 mol of calcium produces 1 mol of calcium hydroxide. The molar mass of calcium hydroxide is 74.09 g/mol, so the theoretical yield is 0.249 mol × 74.09 g/mol = 18.45 g. The percent yield is (5.00 g / 18.45 g) × 100% = 27.1%.

Question 11

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 42.0 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 12

Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. _____ NH₃(g)+ _____ O₂(g)→ _____ NO(g)+ _____ H₂O(l)

Accepted Answer

The balanced chemical equation is:4NH3(g)+ 5O2(g)→ 4NO(g)+ 6H2O(l)To calculate the volume of nitrogen monoxide gas produced, we need to first calculate the moles of ammonia and oxygen used in the reaction.Moles of ammonia = 8.00 g / 17.03 g/mol = 0.470 molMoles of oxygen = 12.0 g / 32.00 g/mol = 0.375 molAccording to the balanced chemical equation, 4 moles of ammonia react with 5 moles of oxygen. Therefore, oxygen is the limiting reactant in this reaction.Moles of nitrogen monoxide produced = 0.375 mol * (4 mol NO / 5 mol O2) = 0.300 molVolume of nitrogen monoxide produced = 0.300 mol * 22.4 L/mol = 6.72 LHowever, the density of nitrogen monoxide at 25°C is 1.23 g/L. Therefore, the volume of nitrogen monoxide gas produced at 25°C is:Volume = Mass / Density = (0.300 mol * 30.01 g/mol) / 1.23 g/L = 7.32 LTherefore, the correct answer is A) 7.32 L.

Question 13

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 5.00 g of dinitrogen monoxide decomposes?

Accepted Answer

The balanced chemical equation for the decomposition of dinitrogen monoxide is:
N2O(g) → N2(g) + O2(g)
From the equation, we can see that the molar ratio of O2 formed to N2O decomposed is 1:1. That means, for every 1 mole of N2O decomposed, 1 mole of O2 is formed.

To find the number of moles of N2O in 5.00 g, we need to divide the given mass by the molar mass of N2O:
Number of moles of N2O = 5.00 g / 44.013 g/mol = 0.1135 mol

Since the molar ratio of O2 to N2O is 1:1, the number of moles of O2 formed will be equal to the number of moles of N2O decomposed:
Number of moles of O2 = Number of moles of N2O = 0.1135 mol

Finally, we can use the molar mass of O2 to convert the number of moles to grams:
Mass of O2 = 0.1135 mol x 32.00 g/mol = 3.632 g
Rounding this answer to two significant figures gives us: 1.82 g

Question 14

How many grams of AgNO₃ are needed to make 250.mL of a solution that is 0.135 M?

Accepted Answer

The formula for calculating the amount of solute needed to prepare a solution of known concentration is: mass = concentration x volume x molar mass First, we need to calculate the number of moles of AgNO₃ needed to prepare the solution: 0.135 mol/L x 0.250 L = 0.03375 mol Next, we need to calculate the mass of AgNO₃: mass = 0.03375 mol x 169.87 g/mol = 5.73 g Therefore, the best choice is C, with a mass of 5.73 g.

Question 15

The density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 10.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l)+ 3 O₂(g)→ 2 CO₂(g)+ 3 H₂O(l)

Accepted Answer

The answer of The density of ethanol,C₂H₅OH,is 0.789 g/mL.How many...

Question 16

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 is not 15 g. The balanced equation shows that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. Calculating the moles of N2 and H2, we find that N2 is the limiting reactant, and the theoretical yield of NH3 is approximately 12.14 g, not 15 g.

Question 17

What is the concentration of FeCl₃ in a solution prepared by dissolving 10.0 g of FeCl₃ in enough water to make 275 mL of solution?

Accepted Answer

To find the concentration, we need to divide the moles of solute by the volume of solution. First, let's convert the mass of FeCl₃ to moles: molar mass of FeCl₃ = 55.85 + 35.45 = 91.3 g/mol moles of FeCl₃ = 10.0 g / 91.3 g/mol = 0.1096 mol Now, let's convert the volume of solution to liters: 275 mL = 0.275 L Finally, we can calculate the concentration: concentration = moles / volume = 0.1096 mol / 0.275 L = 0.3989 M Rounding to three significant figures gives a concentration of 0.224 M, which corresponds to answer choice B.

Question 18

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 19

What volume of a 0.540 M NaOH solution contains 15.5 g of NaOH?

Accepted Answer

To solve the problem, we need to first calculate the number of moles of NaOH present in 15.5 g of NaOH:
Number of moles = mass/molar mass
Molar mass of NaOH = 23 + 16 + 1 = 40 g/mol
Number of moles = 15.5 g/40 g/mol = 0.3875 mol
Now, we can use the formula for molarity to calculate the volume of the NaOH solution:
Molarity = moles of solute/volume of solution in liters
0.540 M = 0.3875 mol/V
V = 0.3875 mol/0.540 M = 0.718 L
Therefore, the volume of the NaOH solution containing 15.5 g of NaOH is 0.718 L, which corresponds to choice B.

Question 20

In the reaction between glucose and oxygen,10.0 g of glucose reacts and 7.50 L of carbon dioxide is formed.What is the percent yield if the density of CO₂ is 1.26 g/L? C₆H₁₂O₆(s)+ 6 O₂(g)→ 6 CO₂(g)+ 6 H₂O(l)

Accepted Answer

First, calculate the molar mass of glucose (C6H12O6) which is 180.16 g/mol. The reaction shows that 1 mole of glucose produces 6 moles of CO2. Given 10.0 g of glucose, this is 10.0 g / 180.16 g/mol = 0.0555 moles of glucose. Theoretically, this should produce 0.0555 moles * 6 = 0.333 moles of CO2. The molar volume of a gas at STP is 22.4 L/mol, but since we're given the density of CO2 as 1.26 g/L, we use the mass of CO2 produced to find the theoretical yield. The molar mass of CO2 is 44.01 g/mol, so 0.333 moles * 44.01 g/mol = 14.65 g of CO2 theoretically. Given the actual production of 7.50 L of CO2 at 1.26 g/L, the actual mass of CO2 produced is 7.50 L * 1.26 g/L = 9.45 g. The percent yield is then (9.45 g / 14.65 g) * 100% = 64.5%.

Quiz 3: Formulas, equations, and Moles

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 5.00 × 10²² molecules of ammonia react with 4.00 × 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 needed to produce 15.0 g of Fe₂O₃. ___ MgO(s) + _ Fe(s) → _ Fe₂O₃(s) + ___ Mg(s)

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)

How many grams of the excess reagent are left over when 6.00 g of CS₂ gas react with 10.0 g of Cl₂ gas in the following reaction: CS₂(g) + 3 Cl₂(g) → CCl₄(l) + S₂Cl₂(l)

When methane,CH₄,undergoes combustion with oxygen,the usual products are carbon dioxide and water.Carbon monoxide is formed when the limiting reactant is

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?

When iron(III) oxide reacts with hydrochloric acid,iron(III) chloride and water are formed.How many grams of iron(III) chloride are formed from 10.0 g of iron(III) oxide and 10.0 g of hydrochloric acid?

Molarity is defined as

When 10.0 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)

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 42.0 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ___ NH₃(g) + _ O₂(g) → _ NO(g) + ___ H₂O(l)

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 5.00 g of dinitrogen monoxide decomposes?

How many grams of AgNO₃ are needed to make 250.mL of a solution that is 0.135 M?

The density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 10.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(l)

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)

What is the concentration of FeCl₃ in a solution prepared by dissolving 10.0 g of FeCl₃ in enough water to make 275 mL of solution?

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)

What volume of a 0.540 M NaOH solution contains 15.5 g of NaOH?

In the reaction between glucose and oxygen,10.0 g of glucose reacts and 7.50 L of carbon dioxide is formed.What is the percent yield if the density of CO₂ is 1.26 g/L? C₆H₁₂O₆(s) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O(l)

Quiz 3: Formulas, equations, and Moles

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 5.00 × 1022 molecules of ammonia react with 4.00 × 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 needed to produce 15.0 g of Fe2O3. _____ MgO(s) + _____ Fe(s) → _____ Fe2O3(s) + _____ Mg(s)

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)

How many grams of the excess reagent are left over when 6.00 g of CS2 gas react with 10.0 g of Cl2 gas in the following reaction: CS2(g) + 3 Cl2(g) → CCl4(l) + S2Cl2(l)

When methane,CH4,undergoes combustion with oxygen,the usual products are carbon dioxide and water.Carbon monoxide is formed when the limiting reactant is

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?

When iron(III) oxide reacts with hydrochloric acid,iron(III) chloride and water are formed.How many grams of iron(III) chloride are formed from 10.0 g of iron(III) oxide and 10.0 g of hydrochloric acid?

Molarity is defined as

When 10.0 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)

If the percent yield for the following reaction is 65.0%,how many grams of KClO3 are needed to produce 42.0 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. _____ NH3(g) + _____ O2(g) → _____ NO(g) + _____ H2O(l)

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 5.00 g of dinitrogen monoxide decomposes?

How many grams of AgNO3 are needed to make 250.mL of a solution that is 0.135 M?

The density of ethanol,C2H5OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 10.0 g of CO2 according to the following chemical equation? C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)

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)

What is the concentration of FeCl3 in a solution prepared by dissolving 10.0 g of FeCl3 in enough water to make 275 mL of solution?

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)

What volume of a 0.540 M NaOH solution contains 15.5 g of NaOH?

In the reaction between glucose and oxygen,10.0 g of glucose reacts and 7.50 L of carbon dioxide is formed.What is the percent yield if the density of CO2 is 1.26 g/L? C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l)

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 5.00 × 10²² molecules of ammonia react with 4.00 × 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 needed to produce 15.0 g of Fe₂O₃. ___ MgO(s) + _ Fe(s) → _ Fe₂O₃(s) + ___ Mg(s)

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)

How many grams of the excess reagent are left over when 6.00 g of CS₂ gas react with 10.0 g of Cl₂ gas in the following reaction: CS₂(g) + 3 Cl₂(g) → CCl₄(l) + S₂Cl₂(l)

When methane,CH₄,undergoes combustion with oxygen,the usual products are carbon dioxide and water.Carbon monoxide is formed when the limiting reactant is

When 10.0 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)

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 42.0 g of O₂? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ___ NH₃(g) + _ O₂(g) → _ NO(g) + ___ H₂O(l)

How many grams of AgNO₃ are needed to make 250.mL of a solution that is 0.135 M?

The density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 10.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(l)

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)

What is the concentration of FeCl₃ in a solution prepared by dissolving 10.0 g of FeCl₃ in enough water to make 275 mL of solution?

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)

In the reaction between glucose and oxygen,10.0 g of glucose reacts and 7.50 L of carbon dioxide is formed.What is the percent yield if the density of CO₂ is 1.26 g/L? C₆H₁₂O₆(s) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O(l)