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(I) The equilibrium partial pressure of NO in the reaction N2(g) + O2(g) ⇌ 2 NO(g) at 800

K is 3.0 x 10-6 Pa. What are the partial pressures of N2 and O2 at equilibrium if K = 3.4 × 10-21 at 800 K?



(II) How should the total volume of the following equilibrium reaction mixture be changed to increase the amount of CO2(g)? C(s) + CO2(g) ⇌ 2 CO(g)


Select one:

A) Total volume should decrease.

B) Total volume should remain the same.

C) There is insufficient information given.

D) Total volume should increase.



(III) Consider the reaction A (aq) + 3 B (aq) ⇌ 2 NH3 (g). If we have 1.0 L and K = 9, calculate Q if the volume is increased to 10.0 L.

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(i) N 2 (g) +... View the full answer

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