Glycine, an amino acid used by organisms to make proteins, is represented by the following molecular model. (a) Write its molecular formula.

Glycine, an amino acid used by organisms to make proteins, is represented by the following molecular model. (c) Calculate how many moles of glycine are in a 100.0-g sample of glycine.

Glycine, an amino acid used by organisms to make proteins, is represented by the following molecular model. (d) Calculate the percent nitrogen by mass in glycine.

The following diagram represents a high-temperature reaction between CH4 and H2O. Based on this reaction, find how many moles of each product can be obtained starting with 4.0 mol CH4.

Based on this reaction, find how many moles of CO can be obtained starting with 4.0 mol CH4?

The following diagram represents a high-temperature reaction between CH4 and H2O. Based on this reaction, find how many moles of each product can be obtained starting with 4.0 mol CH4. Based on this reaction, how many moles of H2 can be obtained starting with 4.0 mol CH4?

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (a) Write the balanced chemical equation for the reaction.

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (d) If so, how many of which type are left over?

How many N2 molecules are left over?

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (d) Are any reactant molecules left over, based on the diagram?

Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (a) How many molecules of NO2 can be formed, assuming the reaction goes to completion?

Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (c) If the actual yield of the reaction was 75% instead of 100%, how many molecules of each kind would be present after the reaction was over?

Write 'true' or 'false' for each statement. (a) We balance chemical equations as we do because energy must be conserved.

Write 'true' or 'false' for each statement. (b) If the reaction 2 O₃(g) → 3 O₂(g) goes to completion and all O₃ is converted to O₂, then the mass of O₃ at the beginning of the reaction must be the same as the mass of O₂ at the end of the reaction.

A key step in balancing chemical equations is correctly identifying the formulas of the reactants and products. For example, consider the reaction between calcium oxide, CaO(s), and H2O1l2 to form aqueous calcium hydroxide. (b) Is it possible to balance the equation if you incorrectly identify the product as CaOH1aq2, and if so, what is the equation?

Balance the following equations: (c) Al(OH)₃(s) + H₂SO₄(l) → Al₂(SO₄)₃(s) + H₂O(l)

Balance the following equations:

(a) HClO₄(aq) + P₄O₁₀(s) → HPO₃(aq) + Cl₂O₇(l)

(b) Au₂S₃(s + H₂(g) → Au(s) + H₂S(g)

Balance the following equations: (c) Ba₃N₂(s) + H₂O(aq) → Ba(OH)₂(aq) + NH₃(g)

Balance the following equations: (d) Na₂CO₃(aq) + HCl(aq) → NaCl(aq) + H₂O(l) + CO₂(g)

Balance the following equations:

(a) CaS(s) + H₂O(l) → Ca(HS₂)₂(aq) + Ca(OH)₂(aq)

(b) NH₃(g) + O₂(g) → NO(g) + H₂O(g)

(c) FeCl₃(s) + Na₂CO₃(aq) → Fe₂(CO₃)₃(s) + NaCl(aq)

(d) FeS₂(s) + O₂(g) → Fe₂O₃(s) + SO₂(g)

Balance the following equations: (a) CF₄(l) + Br₂(g) → CBr₄(l) + F₂(g) (b) Cu(s) + HNO₃(aq) → Cu(NO₃)₂(aq) + NO2(g) + H₂O(l)

Balance the following equations: (c) MnO₂(s) + HCl(aq) → MnCl₂(s) + H₂O(l) + Cl₂(g)

Balance the following equations: (d) KOH(aq) + H₃PO₄(aq) → K₃PO₄(aq) + H₂O(l)

Write balanced chemical equations corresponding to each of the following descriptions: (a) Potassium cyanide reacts with an aqueous solution of sulfuric acid to form hydrogen cyanide gas. (b) When an aqueous solution of ammonium nitrite (NH₄NO₂) reacts with an aqueous solution of potassium hydroxide, ammonia gas, water and metal nitrate is formed. (c) When hydrogen gas is passed over solid hot iron(III) oxide, the resulting reaction produces iron and gaseous water. (d) When liquid ethanoic acid (CH₃COOH) is combusted, carbon dioxide and water are formed.

Write balanced chemical equations to correspond to each of the following descriptions: (a) When sulfur trioxide gas reacts with water, a solution of sulfuric acid forms. (b) Boron sulfide, B₂S₃(s), reacts violently with water to form dissolved boric acid, H₃BO₃, and hydrogen sulfide gas.

Write balanced chemical equations to correspond to each of the following descriptions: (c) Phosphine, PH₃(g), combusts in oxygen gas to form water vapor and solid tetraphosphorus decaoxide.

Write balanced chemical equations to correspond to each of the following descriptions: (d) When solid mercury(II) nitrate is heated, it decomposes to form solid mercury(II) oxide, gaseous nitrogen dioxide, and oxygen. (e) Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper(II) sulfate, sulfur dioxide gas, and water.

(a) When a compound containing C, H, and O is completely combusted in air, what reactant besides the hydrocarbon is involved in the reaction?

(b) What products form in this reaction?

(c) What is the sum of the coefficients in the balanced chemical equation for the combustion of one mole of acetone, C3H6O1l2, in air?