Write and balance the equation for the given reaction. When copper metal reacts with nitric acid to give aqueous copper(II) nitrate, water, nitrogen monoxide as products. Concept Introduction: The chemical reaction in which both oxidation and reduction process takes place is known as redox reaction. In this reaction, transfer of electrons takes place among the elements. Oxidation is the process in which either loss of electrons, oxidation number increases, or loss of hydrogen atoms takes place. An element is oxidized, when oxidation number increases. Reduction is the process in which either gain of electrons, oxidation number decreases, or gain hydrogen atoms takes place. An element is reduced, when oxidation number decreases. The balanced chemical equation is the equation in which number of different atoms of elements in the reactants side is similar to the product side.

Question

Exercise: At 373 K, the equilibrium constant for the reaction COCl2(g) D CO(g) + Cl2(g) is 2.9x10-10. The concentrations of the gases in a 1-L reaction flask are [COCl2]= 3.50x10-3 M, [Cl2]=3.25x10-6 M, and [CO]=1.11x10-5 M. (a) Is the mixture of gases at equilibrium? Answer should be supported with calculations. (b) If not, which direction will the reaction proceed to reach equilibrium?

Answer 1

Question

Chapter 18.4, Problem 18.4SC

Interpretation Introduction

Interpretation:

Write and balance the equation for the given reaction.

When copper metal reacts with nitric acid to give aqueous copper(II) nitrate, water, nitrogen monoxide as products.

Concept Introduction:

The chemical reaction in which both oxidation and reduction process takes place is known as redox reaction. In this reaction, transfer of electrons takes place among the elements.

Oxidation is the process in which either loss of electrons, oxidation number increases, or loss of hydrogen atoms takes place. An element is oxidized, when oxidation number increases.

Reduction is the process in which either gain of electrons, oxidation number decreases, or gain hydrogen atoms takes place. An element is reduced, when oxidation number decreases.

The balanced chemical equation is the equation in which number of different atoms of elements in the reactants side is similar to the product side.

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Exercise: At 373 K, the equilibrium constant for the reaction COCl2(g) D CO(g) + Cl2(g) is 2.9x10-10. The concentrations of the gases in a 1-L reaction flask are [COCl2]= 3.50x10-3 M, [Cl2]=3.25x10-6 M, and [CO]=1.11x10-5 M. (a) Is the mixture of gases at equilibrium? Answer should be supported with calculations. (b) If not, which direction will the reaction proceed to reach equilibrium?

Practice Exercise 1If you complete and balance the following oxidation–reduction reaction in basic solutionNO2-(aq)+ Al(s)---->NH3(aq) + Al(OH)4-(aq) how many hydroxide ions are there in the balanced equation(for the reaction balanced with the smallest whole-numbercoefficients)?(a) One on the reactant side (b) One on the product side(c) Four on the reactant side (d) Seven on the product side(e) None