Introductory Chemistry, v. 1.0

How many molecules of O₂ will react with 6.022 × 10²³ molecules of H₂ to make water? The reaction is 2H₂(g) + O₂(g) → 2H₂O(ℓ).

How many molecules of H₂ will react with 6.022 × 10²³ molecules of N₂ to make ammonia? The reaction is N₂(g) + 3H₂(g) → 2NH₃(g).

How many moles are present in 6.411 kg of CO₂? How many molecules is this?

How many moles are present in 2.998 mg of SCl₄? How many molecules is this?

What is the mass in milligrams of 7.22 × 10²⁰ molecules of CO₂?

What is the mass in kilograms of 3.408 × 10²⁵ molecules of SiS₂?

What is the mass in grams of 1 molecule of H₂O?

What is the mass in grams of 1 atom of Al?

What is the volume of 3.44 mol of Ga if the density of Ga is 6.08 g/mL?

What is the volume of 0.662 mol of He if the density of He is 0.1785 g/L?

For the chemical reaction

2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(ℓ)

assume that 13.4 g of C₄H₁₀ reacts completely to products. The density of CO₂ is 1.96 g/L. What volume in liters of CO₂ is produced?

For the chemical reaction

2GaCl₃(s) + 3H₂(g) → 2Ga(ℓ) + 6HCl(g)

if 223 g of GaCl₃ reacts completely to products and the density of Ga is 6.08 g/mL, what volume in milliliters of Ga is produced?

Calculate the mass of each product when 100.0 g of CuCl react according to the reaction

2CuCl(aq) → CuCl₂(aq) + Cu(s)

What do you notice about the sum of the masses of the products? What concept is being illustrated here?

Calculate the mass of each product when 500.0 g of SnCl₂ react according to the reaction

2SnCl₂(aq) → SnCl₄(aq) + Sn(s)

What do you notice about the sum of the masses of the products? What concept is being illustrated here?

What mass of CO₂ is produced from the combustion of 1 gal of gasoline? The chemical formula of gasoline can be approximated as C₈H₁₈. Assume that there are 2,801 g of gasoline per gallon.

What mass of H₂O is produced from the combustion of 1 gal of gasoline? The chemical formula of gasoline can be approximated as C₈H₁₈. Assume that there are 2,801 g of gasoline per gallon.

A chemical reaction has a theoretical yield of 19.98 g and a percent yield of 88.40%. What is the actual yield?

A chemical reaction has an actual yield of 19.98 g and a percent yield of 88.40%. What is the theoretical yield?

Given the initial amounts listed, what is the limiting reagent, and how much of the other reactants are in excess?

$$\underset{\text{35}.0\text{ g}}{{\text{P}}_{\text{4}}}+\underset{\text{12}.\text{7 g}}{\text{3NaOH }}+\underset{\text{9}.\text{33 g}}{{\text{3H}}_{\text{2}}\text{O}}\to {\text{2Na}}_{\text{2}}{\text{HPO}}_{\text{4}}+{\text{PH}}_{\text{3}}$$

Given the initial amounts listed, what is the limiting reagent, and how much of the other reactants are in excess?

$$\underset{\text{46}.\text{3 g}}{{\text{2NaCrO}}_{\text{2}}}+\underset{\text{88}.\text{2 g}}{{\text{3NaBrO}}_{\text{4}}}+\underset{\text{32}.\text{5 g}}{\text{2NaOH}}\to {\text{3NaBrO}}_{\text{3}}+{\text{2Na}}_{\text{2}}{\text{CrO}}_{\text{4}}+{\text{H}}_{\text{2}}\text{O}$$

Verify that it does not matter which product you use to predict the limiting reagent by using both products in this combustion reaction to determine the limiting reagent and the amount of the reactant in excess. Initial amounts of each reactant are given.

$$\underset{\text{26}.\text{3 g}}{{\text{C}}_{\text{3}}{\text{H}}_{\text{8}}}+\underset{\text{21}.\text{8 g}}{{\text{5O}}_{\text{2}}}\to {\text{3CO}}_{\text{2}}\text{(g)}+{\text{4H}}_{\text{2}}\text{O(}\ell \text{)}$$

Just in case you suspect Exercise 21 is rigged, do it for another chemical reaction and verify that it does not matter which product you use to predict the limiting reagent by using both products in this combustion reaction to determine the limiting reagent and the amount of the reactant in excess. Initial amounts of each reactant are given.

$$\underset{\text{35}.0\text{ g}}{{\text{2P}}_{\text{4}}}+\underset{\text{12}.\text{7 g}}{\text{6NaOH }}+\underset{\text{9}.\text{33 g}}{{\text{6H}}_{\text{2}}\text{O}}\to 3{\text{Na}}_{\text{2}}{\text{HPO}}_{\text{4}}+5{\text{PH}}_{\text{3}}$$