Answer these questions (R = shift right. L = shift left. NC = no change) regardi

Question

Answer these questions (R = shift right. L = shift left. NC = no change) regarding the following endothermic process 3H_2(g) + N_2(g) doubleheadarrow 2NH_3(g) What effect would removing NH_3 from the flask have on equilibrium? What effect would decreasing the size of the flask have on equilibrium? What is the effect of raising the temperature? What effect does increasing the partial pressure of H_2 have on equilibrium? what effect does adding a catalyst have on equilibrium? At 450 degree C., K_p = 2.0 times 10^-6, for the reaction 2 C0_2 (g) 2 CO (g) + 0_2 (g) If only 4.0 at of pure carbon dioxide is initially present, calculate the equilibrium pressures of a species. What is the numerical value of:K_c?__Initial Q? When the following reaction comes to equilibrium, will the concentrations of the reactants Does the answer to this question depend on the initial consent the and product? a(g) + b(g) 2 c(g) k_c = 1.4 times 10^-5

Explanation / Answer

2.(5)

3H2(g) + N2(g) <===> 2 NH3(g)

according lechatliers principle " a system at equilibrium undergoes stress.the equilibrium shifts in such a way that ,

in order to un do the stress"

a. removal of NH3 shifts equilibrium towards products side. = R

b. decreasing size,volume decreases,so that equilibrium towards products side. = R

c. as the reaction is endothermic, increasing temperature shifts equilibrium towards products = R

d. if H2 partial pressure increases, shifts equilibrium towards products = R

e. no effect, catalyst do not alters equilibrium.

3)

b) kp = kc(RT)^Dn

Dn = nproducts - nreactants

   = 3-2 = 1

2*10^-6 = x(0.0821*723)^1

x = Kc = 3.37*10^-8

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