Calculate the equilibrium constant K at 298 K for the following reaction:
3C2H2 → C6H6
?G f^o(C2H2) = 209.2 kJ/mol, ?G f^o(C6H6) = 129.7kJ/mol
Choices:
a.) 3.33*10^95
b.) 2.57*10^45
c.) 6.53 * 10^30
d.) 1.96*10^87
Calculate the equilibrium constant K at 298 K for the following reaction: 3C2H2 → C6H6 ?G...
Determine the equilibrium constant for the following reaction at 298 K: SO3(g) + H2O(g) → H2SO4(l) ΔG°rxn = -90.5 kJ mol-1 Group of answer choices 0.964 4.78 × 1011 7.31 × 1015 1.37 × 10-16 9.11 × 10-8
ΔH0 (kJ/mol) C2H2 (g) = 226.7 C6H6 (g) = 82.9 S0(J/mol*K) C2H2 (g) = 200.8 C6H6 (g) = 269.2 Cp C2H2 (g) Cp = 30.7 + 5.28*10-2 T + 1.63*10-5 T2 (J/mol*K) C6H6 (g) Cp = -1.7 + 3.25 *10-2 T - 11.06*10-5 T2 (J/mol*K) Compute ΔH(Temperature Final)reaction and ΔS(Temperature Final)reaction Initial Temperature = 298.15K Final Temperature = 330K
The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘ ΔG∘=−RTlnK where T is a specified temperature in kelvins (usually 298 KK) and R is equal to 8.314 J/(K⋅mol) Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as KK except that the concentrations or pressures used are not necessarily the equilibrium values. Part A Acetylene, C2H2,...
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
The equilibrium constant, Kp, for the following reaction is 0.160 at 298 K. Calculate K, for this reaction at this temperature. 2NOBr(g) 2NO(g) + Br2(g) Kc =
1
2
Part A Calculate Kp at 298 K for the reaction NO(g) + + O2(g) → NO2 (g) assuming that AH is constant over the interval 298-600 K. Kp = 2.31x106 Submit Previous Answers ✓ Correct Part B Calculate Kp at 477 K for this reaction assuming that AHR is constant over the interval 298-600 K. PO AQ * o o ? Kp = | Submit Previous Answers Request Answer Revie For the reaction 2CH4 (g) = C2H2(g) +...
The equilibrium constant, Kp, for the following reaction is 6.25 at 298 K. 2NO(g) + Br2(g) 2NOBr(g) If ΔH° for this reaction is -16.1 kJ, what is the value of Kp at 187 K? Kp =
The equilibrium constant, Ky, for the following reaction is 0.110 at 298 K. NH_HS(s) NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.50 L container at 298 K contains 2.94 mol of NH_HS(s) and 0.219 mol of NH3(g), the partial pressure of H2S(g) is atm.
Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) → ClO(g) + O2(g) ΔG° = - 34.5 kJ Please explain how you enter it into the calculator I get 1.23*10^-14. Which is incorrect the answer is 1.12*10^-6.
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 212 K? Kp =