The following endothermic reaction is at equilibrium at a pressure of 1 atm, in

Question

The following endothermic reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaHCO_3(s) NaOH(s) + CO_2(g) Which, if any, of the following actions will increase the amount of CO_2 gas present at equilibrium? Consider the following reaction: 2NO(g) + O_2(g) 2NO^2(g) Delta H_rxn degree = -114 kJ Under which reaction conditions would you expect to produce the largest amount of NO_2? The reaction shown below is at equilibrium. Use Le Chatelier's principle to predict the effect of removing NH_3 from the equilibrium reaction mixture. N_2(g) + 3H_2(g) 2NH_3

Explanation / Answer

6) C) if the volume is increased there will be an instant drop in pressure and the equilibrium is disturbed, so once again equilibrium is set up by increasing the volume of CO2 only so reaction move forward so the CO2 concentration increses.

7) b) Enthalpy of this reactions are less than zero, and are therefore exothermic reaaction when reaction is forwarded.

Means reducing the heat the reactin would go forward, because heat is liberated in the reaction.

2 moleof gas on left side reduced to the 1 mole on th right side, means by compressing the gas or increasing the pressure of the gas result in the increased product concentration because to sustain the increased pressure concetraion of species on right occupy less voume on right, so the reaction go forward.

8) B) Unreacted hydrogen and nitrogen gases are then returned to equilibrium by moving reaction forward.

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