1
answer
0
watching
372
views
18 Nov 2019
The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + 2B(g) doubleheadarrow AB_2(g) K_c = 59 AB_2(g) + B(g) doubleheadarrow AB_3(g) K_c = ? A(g) + 3B(g) doubleheadarrow AB_3(g) k_c = 478 3.5 times 10^-5 2.8 times 10^4 8.1 0.12 89 The reaction below has a K_p value of 3.3 times 10^-5. What is the value of K_c for this reaction at 700 K? 2 SO_3(g) doubleheadarrow 2 SO_2(g) + O_2(g) 5.7 times 10^-7 1.7 times 10^6 C) 3.3 times 10^-5 D) 3.0 times 10^4 1.9 times 10^-3 Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows [P_4O_10]_eq = 2.000 moles, [P4]_eq = 3.000 moles, [O_2]_eq = 4.000 M P_4O_10 (s) doubleheadarrow P_4(s) + 5 O_2(g) 20.00 4.000 1.320 1536 1024
The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + 2B(g) doubleheadarrow AB_2(g) K_c = 59 AB_2(g) + B(g) doubleheadarrow AB_3(g) K_c = ? A(g) + 3B(g) doubleheadarrow AB_3(g) k_c = 478 3.5 times 10^-5 2.8 times 10^4 8.1 0.12 89 The reaction below has a K_p value of 3.3 times 10^-5. What is the value of K_c for this reaction at 700 K? 2 SO_3(g) doubleheadarrow 2 SO_2(g) + O_2(g) 5.7 times 10^-7 1.7 times 10^6 C) 3.3 times 10^-5 D) 3.0 times 10^4 1.9 times 10^-3 Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows [P_4O_10]_eq = 2.000 moles, [P4]_eq = 3.000 moles, [O_2]_eq = 4.000 M P_4O_10 (s) doubleheadarrow P_4(s) + 5 O_2(g) 20.00 4.000 1.320 1536 1024
Hubert KochLv2
11 Mar 2019