Calculate how many moles of NO₂ form when each quantity of reactant completely reacts. 2 N₂O₅( g) → 4 NO₂(g) + O₂(g) a. 2.5 mol N₂O₅

Consider the balanced equation:

SiO₂(s) + 3 C(s) → SiC(s) + 2 CO(g)

Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.

Hydrobromic acid dissolves solid iron according to the reaction:

Fe(s) + 2 HBr(aq) → FeBr₂(aq) + H₂(g)

What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock?

Sulfuric acid dissolves aluminum metal according to the reaction:

2 Al(s) + 3 H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3 H₂( g)

Suppose you want to dissolve an aluminum block with a mass of 15.2 g. What minimum mass of H₂SO₄ (in g) do you need? What mass of H₂ gas (in g) does the complete reaction of the aluminum block produce?

For each of the acid–base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. b. 2 HNO₃(aq) + Ca(OH)₂(aq) → 2 H₂O(l) + Ca(NO₃)₂(aq)

Find the limiting reactant for each initial amount of reactants.

2 Na(s) + Br₂(g) → 2 NaBr(s)

a. 2 mol Na, 2 mol Br₂

b. 1.8 mol Na, 1.4 Br₂

c. 2.5 mol Na, 1 mol Br₂

d. 12.6 mol Na, 6.9 mol Br₂

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O₂( g) → 2 Al₂O₃(s)

a. 1 mol Al, 1 mol O₂

b. 4 mol Al, 2.6 mol O₂

c. 16 mol Al, 13 mol O₂

d. 7.4 mol Al, 6.5 mol O₂

Consider the reaction: 4 HCl(g) + O₂(g) → 2 H₂O(g) + 2 Cl₂(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl₂ form from the reaction mixture that produces the greatest amount of products?

Calculate the theoretical yield of the product (in moles) for each initial amount of reactants.

Ti(s) + 2 Cl₂(g) → TiCl₄(s)

a. 4 mol Ti, 4 mol Cl₂

b. 7 mol Ti, 17 mol Cl₂

c. 12.4 mol Ti, 18.8 mol Cl₂

Calculate the theoretical yield of product (in moles) for each initial amount of reactants.

3 Mn(s) + 2 O₂(g) → Mn₃O₄(s)

a. 3 mol Mn, 2 mol O₂

b. 4 mol Mn, 7 mol O₂

c. 27.5 mol Mn, 43.8 mol O₂

Zinc sulfide reacts with oxygen according to the reaction: 2 ZnS(s) + 3 O₂(g) → 2 ZnO(s) + 2 SO₂( g) A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O₂. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl₂(s) + H₂S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl₂(s) + H₂S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. 2 Al(s) + 3 Cl₂(g) → 2 AlCl₃(s) c. 0.235 g Al, 1.15 g Cl₂

For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F₂( g) → TiF₄(s) c. 0.233 g Ti, 0.288 g F₂

Iron(III) oxide reacts with carbon monoxide according to the equation: Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) A reaction mixture initially contains 22.55 g Fe₂O₃ and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Elemental phosphorus reacts with chlorine gas according to the equation: P₄(s) + 6 Cl₂( g) → 4 PCl₃(l) A reaction mixture initially contains 45.69 g P₄ and 131.3 g Cl₂. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O₂(g) → 2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O₂, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Urea (CH₄N₂O) is a common fertilizer that is synthesized by the reaction of ammonia (NH₃) with carbon dioxide: 2 NH₃(aq) + CO₂(aq) → CH₄N₂O(aq) + H₂O(l) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

Many computer chips are manufactured from silicon, which occurs in nature as SiO₂. When SiO₂ is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO₂ reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the percent yield for the reaction.