Write the equilibrium constant expressions for the following systems CaCO_3(s) CaO(s) + CO_2(g) 3Fe(s) + 4H_2O(g)...

Question

Question

Write the equilibrium constant expressions for the

Answer 1

Answer #1

While writing expression for Kp , solid species cannot be considered.

Kp = equilibrium partial pressure of products/ equilibrium partial pressure of reactants

5) A) Kp = P_CO2 P = partial pressure at equilibrium

B) Kp = (P_H2)⁴ / (P_H2O)⁴

C) Kp = P_O2

6) For given reaction

Δn = no of moles of products - no of moles of reactants = 3-5 = -2

If volume decreased, equilibrium shifts to right.

If pressure decreased, equilibrium shifts to left.

Answer 2

Similar Homework Help Questions

CaCO_3(s) <-> CaO (s) + CO_2 (g) what direction will the reaction shift if we remove...

CaCO_3(s) <-> CaO (s) + CO_2 (g) what direction will the reaction shift if we remove ALL CaO (s)? What direction will the reaction shift if we add CaCO_3 (s)? Please explain, thank you!
Write the equilibrium constant expressions for K_c for the following reactions: 2NO_2(g)+7H_2(g) equivalent 2NH_3(g)+4H_2O(l) 2ZnS(s)+3O_2(g) equivalent...

Write the equilibrium constant expressions for K_c for the following reactions: 2NO_2(g)+7H_2(g) equivalent 2NH_3(g)+4H_2O(l) 2ZnS(s)+3O_2(g) equivalent 2ZnO(s)+2SO_2(g) C(s)+CO_S(g) equivalent 2CO(g) C_6H_5COOH(aq) equivalent C_6H_5COO^-(aq)+H^+(aq)
At elevated temperatures, BrF_5 establishes the following equilibrium. 2BrF_5(g) Br_2(g) + 5F_2(g) The equilibrium concentrations of...

At elevated temperatures, BrF_5 establishes the following equilibrium. 2BrF_5(g) Br_2(g) + 5F_2(g) The equilibrium concentrations of the gases at 1500 K are 0.0064 mol/L for BrF_5, 0.0018 mol/L for Br_2, and 0.0090 mol/L for F_o. Calculate the value of K_r. The reaction of iron and water vapor results in an equilibrium 3Fe(s) + 4H_2O(g) Fe_3O_4(s) + 4H_2(g) and an equilibrium constant, K_c, of 4.6 at 850 degree C. What is the concentration of hydrogen present at equilibrium if the reaction...

Consider the following reaction: Ca(s) + 2 H_2O(l) rightarrow Ca(OH)_2(s) + H_2(g) Calculate the heat of...

Consider the following reaction: Ca(s) + 2 H_2O(l) rightarrow Ca(OH)_2(s) + H_2(g) Calculate the heat of reaction based on the following information: 2H_2(g) + O_2(g) rightarrow 2 H_2O(l) DeltaH = -572 kJ/mol CaO(s) + H_2O(l) rightarrow Ca(OH)_2(s) DeltaH = -64 kJ/mol CaCO_3(s) rightarrow CaO(s) + CO_2(g) DeltaH = +178.1 kJ/mol 2 Ca (s) + O_2(g) rightarrow 2 CaO(s) DeltaH = -1270 kJ/mol 13. Acetylene is used in blow torches, and bums according to the following equation: 2 C_2H_2(g) + 5...
What is the entropy change if 4.500 g of CaCO_3(s) is placed in a container and...

What is the entropy change if 4.500 g of CaCO_3(s) is placed in a container and allowed to decompose to CaO(s) and CO_2(g) according to the following reaction?
Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation:2NF_3(g) N_2(g) +...

Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation:2NF_3(g) N_2(g) + 3F_2(g) When 1.82 mol of NF_3, is placed in a 3.00 L container and allowed to come to equilibrium at 800 K, the mixture is found to contain 0.0261 mol of N_2. What is the value of k_p, at this temperature? 398 times 10^-4 1.91 times 10^-5 1.80 times 10^-3 4.43 times 10^-7 3.87 times 10^-4 A red blood cell placed in pure water...

What molar ratio Write a balanced chemical equation which corresponds to the following equilibrium constant question...

What molar ratio Write a balanced chemical equation which corresponds to the following equilibrium constant question K = [NO^-_2] [H_3O^+]/[HNO_2] HNO_2(aq) + H_2O(l) NO^-_2(aq) + H_3O^+(aq) NO^-_2(aq) + H_3O^+(aq) HNO_2(aq) + H_2O(l) NO^-_2 (aq) + H_3O^+(aq) HNO_2(aq) + H_2O(l) NO^-_2 (aq) + H_3O^+(aq) HNO_2(aq) H^+(aq) + OH^-(aq) H_2O(l) HNO_2(aq) NO^-_2 (aq) + H_3O^+(aq) For the equilibrium PCl_5(g) PCl_3(g) + Cl_2(g), K_c = 4.0 at 228 degrees C. If pure PCl_5 is placed in a 1,00-L container and allowed to come...
Determine the equilibrium constant for the following reaction at 527 K. 2Hg(g)+O2(g)-->2HgO(g) Delta H^o= -304.2 kJ...

Determine the equilibrium constant for the following reaction at 527 K. 2Hg(g)+O2(g)-->2HgO(g) Delta H^o= -304.2 kJ and Delta S^o= -414.2 J/K
1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO...

1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO s)+ SO2(8)+ 02(g CH,COO (aq) + H20 (aq) C H,COOH(aq) + H2O(I) 2) The reaction 2HBr(g) H2(g)+ Br2(g) has a Ke value of 1.05 at 25°C. If [HBr] = 0.177 M, [H] 0.223 M and [Br] =0.111 M, in which direction will the system shift?

For which of the following systems at equilibrium and at constant temperature will decreasing the volume...

For which of the following systems at equilibrium and at constant temperature will decreasing the volume cause the equilibrium to shirt to the right? NH_4CI(s) NH_3(g) + HCl(g) 2NO_2(g) 2NO(g) + O_2(g) H_2(g) + Cl_2(g) 2HCl(g) N_2(g) + 3H_2(g) 2NH_3(g) 2H_2O(g) 2H_2(g) + O_2(g)