Write the equilibrium expression for the reaction: 2CO(g) CO_2(g) + C(s), Delta
ID: 492733 • Letter: W
Question
Write the equilibrium expression for the reaction: 2CO(g) CO_2(g) + C(s), Delta H degree = -170 kJ/mol Using: N_2(g) + O_2(g) 2NO(g); K = 4.1 times 10^-31 Determine K for: N_2(g) + 1/2O_2(g) N_2O(g); K = 2.4 times 10^-18 2NO(g) N_2O(g) + 1/2O_2(g) Is the following reaction exothermic or endothermic? N_2(g) + 3H_2(g) 2NH_3(g); K_P(300 degree C) = 4.34 times 10^-3 and K_p(600 degree C) = 2.25 times 10^-6 The following diagrams represent the equilibrium state for three different reactions. Which reaction has the largest equilibrium constant of the three reactions? Which reaction has the smallest?Explanation / Answer
2) the reaction is 2CO(g) <------> CO2(g) + C(s)
The equilibrium expression is
Kc = [CO2] /[CO]2
and Kp = PCO2 / [PCO]2
3)The rxn 1 is N2 + O2 ----> 2NO , K1 = 4.1 x1010
rxn 2 is N2 +1/2 O2 ----->N2O K2 = 2.4x10-18
The required reaction 2NO -----> N2O + 1/2 O2
It can be obtained by rxn 2 - rxn 1 and K3= K2/K1
Thus K3 = 2.4x10-18 / 4.1 x 1010
= 5.8 x10-9
4) For the give reaction Keq at 300 C is 4.34x103 nd at 600C it is 2.25x102
Thus with increase in temperature, the K value decreases , hence the reaction is exothermic.
5)The third reaction is the one with largest K value as it has 3 product molecules and two reactant molecules.
The second one is the one with smallest K value as it has only one product and 3 each of reactant molecules.
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