3. Nitrogen dioxide dimerizes according to the following reaction: K-6.7 A 2.25-

Question

3. Nitrogen dioxide dimerizes according to the following reaction: K-6.7 A 2.25-L container contains 0.055 mol of NO2 and 0.082 mol of N 0s at 298 K. Is the reaction at equilibrium? If not, in what direction will the reaction proceed? 4. Consider the following reaction: NHaHS(s) NH3(g) + H2S(g) At a certain temperature, Kc 8.5 x 103. A reaction mixture at this temperature containing solid NH4HS has [NHa] 0.166 M and [H2S 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached? 5. Consider the following reaction: A reaction mixture is made containing an initial [SO Ch] of 2.3x102 M At equilibrium, [Cl2] 1.3x102 M. Calculate the value of the equilibrium constant.

Explanation / Answer

3)

Step 1: find pressure of NO2
Given:
V = 2.25 L
n = 0.055 mol
T = 298.0 K

use:
P * V = n*R*T
P * 2.25 L = 0.055 mol* 0.08206 atm.L/mol.K * 298 K
P = 0.5978 atm

Step 2: find pressure of N2O4
Given:
V = 2.25 L
n = 0.082 mol
T = 298.0 K

use:
P * V = n*R*T
P * 2.25 L = 0.082 mol* 0.08206 atm.L/mol.K * 298 K
P = 0.8912 atm

step 3:
Qp = p(N2O4) / p(NO2)^2
= (0.8912)/(0.5978)^2
= 2.5

Since QP is less than Kp, the reaction is not at equilibrium and it will proceed to the right to reach equilibrium

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