Use your textbook to look up any data (e.g. K_a values) you need to solve these

Question

Use your textbook to look up any data (e.g. K_a values) you need to solve these problems and answer them on a separate sheet of paper. Will the following reaction favor reactants or products: 2 NOCl (g) doubleheadarrow 2 NO (g) + Cl_2 (g) K = 1.6 Times 10^-5 2 CO(g) + O_2 (g) doubleheadarrow 2 CO_2 (g) K = 5.0 Times 10^5 Determine the value of the equilibrium constants for the reverse reactions in problem #1 above. Consider the reaction: 2 NO_2 (g) + O_2 (g) doubleheadarrow NO(g) + O_3 (g) K = 1.7 Times 10^33 Determine the concentration of all species at equilibrium, if you start with: 1.0 M NO and 1.0 M O_3 1.0 M NO_2 and 1.0 M O_2 2.0 M NO_2 and 1.0 M O_2 Given K = 50.2 for the reaction at 445 degree C: H_2 (g) + I_2(g) doubleheadarrow 2 HI (g), determine K for the following reactions: 1/2 H_2 (g) + 1/2 I_2 (g) doubleheadarrow HI(g) HI(g) doubleheadarrow 1/2 H_2 (g) + 1/2 I_2 (g) Determine K for the following reaction: 1/2 N_2 (g) + 1/2 O_2 (g) + 1/2 Br_2 (g) doubleheadarrow NOBr (g) Given: 2 NO (g) doubleheadarrow N_2 (g) + O_2 (g) K = 2.4 Times 10^30 NO(g) + 1/2 Br_2 (g) doubleheadarrow NOBr(g) K = 1.4 Calculate the pH and percent dissociation for 0.020 M monochloroacetic acid. Write net ionic equations to show what happens when aqueous HCl is added to aqueous potassium nitrite aqueous sodium hydroxide is added to aqueous methylamine hydrochloride aqueous sodium hydroxide is added to aqueous nitrous acid For each reaction in problem 7 (a, b & c), Classify each reactant as an acid or a base; Calculate K; Specify whether it favors reactants, products or neither. Calculate the pH of the following salt solutions: 0.20 M KCN 0.50 M methylamine hydrobromide 0.20 M Li_2 CO_3

Explanation / Answer

(1)

We know that K= products / reactants

If K >1 , more products than reactants, K<1 more reactants than products.

for (a) K <1 .So, reactants are favoured

for (b) K>1 .So, products are favoured

(2)

For reverse reaction , Knew =1/ K old

for equation (a) K new =1 / 1.6x10-5 =6.3 x104

for equation (b) K new = 1/ 5 x105 =2 x 10-6

(3)

1 mol NO and 1 mol O3

K= 1.7 x 1033 = NO x O3 / (NO2) x(O2)

1.7 x 1033 = (1+x)*(1+x)/ ((x)*(x))

Solve for x and calculate NO2 and O2 values as 2.43 x 10-17

Chegg rules only one question should be answered.pls post remaining questions separately

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