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. Mol siO2 Mol C Mol SiC Mol CO _____ 1.55 _____ _____

Sulfuric acid is a component of acid rain formed when gaseous sulfur dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous sulfuric acid. Write the balanced chemical equation this reaction. (Note: this is a simplified representation of this reaction.)

Nitric acid is a component of acid rain that forms when gaseous nitrogen dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous nitric acid. Write the balanced chemical equation for this reaction. (Note: this is a simplified representation of this reaction.)

When iron rusts, solid iron reacts with gaseous oxygen to form solid iron(III) oxide. Write the balanced chemical equation for this reaction.

Write the balanced chemical equation for the fermentation of sucrose (C12H22O11) by yeasts in which the aqueous sugar reacts with water to form aqueous ethanol (C2H5OH) and carbon dioxide gas.

Write the balanced chemical equation for each reaction. a. Solid lead(II) sulfide reacts with aqueous hydrobromic acid to form solid lead(II) bromide and dihydrogen monosulfide gas.

Write the balanced chemical equation for each reaction. b. Gaseous carbon monoxide reacts with hydrogen gas to form gaseous methane (CH4) and liquid water.

Write the balanced chemical equation for each reaction. c. Aqueous hydrochloric acid reacts with solid manganese(IV) oxide to form aqueous manganese(II) chloride, liquid water, and chlorine gas.

Write the balanced chemical equation for each reaction. d. Liquid pentane (C5H12) reacts with gaseous oxygen to form carbon dioxide and liquid water.

Write the balanced chemical equation for each reaction. a. Solid copper reacts with solid sulfur to form solid copper(I) sulfide.

Write the balanced chemical equation for each reaction. b. Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water.

Write the balanced chemical equation for each reaction. d. Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water.

Write the balanced chemical equation for the reaction of aqueous potassium hydroxide with aqueous iron(III) chloride to form solid iron(III) hydroxide and aqueous potassium chloride.

Balance each chemical equation. b. Co(NO3)3(aq) + (NH4)2S(aq)¡Co2S3(s) + NH4NO3(aq)

Consider the unbalanced equation for the neutralization of acetic acid: HC₂H₃O₂(aq) + Ba(OH)₂(aq) → H₂O(l) + Ba(C₂H₃O₂)₂(aq) Balance the equation and determine how many moles of Ba(OH)₂ are required to completely neutralize 0.461 mole of HC₂H₃O₂.

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

Calculate how many moles of NH₃ form when each quantity of reactant completely reacts. 3 N₂H₄(l) → 4 NH₃(g) + N₂(g) c. 65.3 g N₂H₄

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. Mol siO2 Mol C Mol SiC Mol CO _____ _____ _____ 10

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. Mol siO2 Mol C Mol SiC Mol CO _____ 1.55 _____ _____

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? What mass of H₂ would the complete reaction of the iron bar produce?

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?

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. d. 2 Sr(s) + O₂(g) → 2 SrO(s)

Find the limiting reactant for each initial amount of reactants. 2 Na(s) + Br₂( g) → 2 NaBr(s) c. 2.5 mol Na, 1 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?

Consider the reaction: 2 CH₃OH(g) + 3 O₂( g) → 2 CO₂( g) + 4 H₂O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO₂ molecules 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) b. 7 mol Ti, 17 mol Cl₂

Calculate the theoretical yield of product (in moles) for each initial amount of reactants. 3 Mn(s) + 2 O₂( g) → Mn₃O₄(s) b. 4 mol Mn, 7 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?