Part A Which of the following actions will cause the equilibrium to shift such t

Question

Part A Which of the following actions will cause the equilibrium to shift such that the partial pressure of NO gas will increase? 2NO(g) + O2(g) = 2NO2(g) H = -13.1 kJ

Which of the following actions will cause the equilibrium to shift such that the partial pressure of gas will increase? Increase the pO2(g)

Decrease the pNO2(g)

Increase the volume

Lower the reaction temperature

Part B Which equilibrium reaction will experience the largest shift towards the reactants in equilibrium position when the overall pressure is increased?

2NO(g) + Br2(g) = 2NOBr(g)

H2(g) + I2(g) = 2HI(g)

2CO2(g) = 2CO(g)+ O2(g)

2NO(g) = N2(g)+ O2(g)

Part C When this reaction in equilibrium is heated, a red/brown color persists. What is true about this reaction? 2NO2(g) = N2O4(g) brown/red colorless When this reaction in equilibrium is heated, a red/brown color persists. What is true about this reaction? brown/red colorless

The increase in T results in a high K value.

The reaction is exothermic. .

Explanation / Answer

Part A) Lower the reaction temperature

Part B) 2CO2(g) = 2CO(g)+ O2(g)

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