Question

Listed in the table are forward and reverse rate constants for the reaction: 2NO(g)
kf
��
kr
�� N2(g) + O2(g)
Temperature (K) Kf (M-1s-1) Kr (M-1s-1)
1400 0.29 1.1×10-6
1500 1.3 1.4×10-5
(a) Determine a value for the equilibrium constant at each temperature {4 points}
(b) Is this reaction exothermic or endothermic? {1 points}

Ammonia reacts with carbon dioxide to form a solid, NH4CO2NH2 according to the following reaction:
2NH3(g) + CO2(g) ⇌ NH4CO2NH2(s)
Where Kp = 0,614 (atm-3) at 298 K. If equilibrium is established at 298 K by starting with pure solid, what is the partial
pressures of NH3 and CO2 at equilibrium? What is the total pressure at equilibrium?

tal Listed in the table are forward and reverse rate constants for the reaction2NO() N,(R)+0,8 Temperature (K) Kt M'S rthe「 1400 1500 0.29 1.3 1.1×106 (a) Determine a value for the equilibrium constant at each temperature i4pri (b) is this reaction exothermic or endothermic? tt painst