Question

The following reaction was allowed to come to equilibrium at 35 degree C. The initial molar concentration for SO_3 is 0.675 M ([SO_3| = 0.675 M) and the initial molar concentration for CO_2 is 0.444 M (|CO_2] = 0.444 M). After the reaction reached equilibrium the concentration of CO_2 now equals 0.214 M ((CO_2] = 0.214 M). What is the K_c value for the reaction? 0.00987 0.0342 7.31 11.8 16.7 At 35 degree C the equilibrium constant value (K_c) for the following reaction is measured at 1.6 times 10^-5. An equilibrium mixture was found to have the following concentrations of Cl_2 and NOCl: [Cl_2] = 0.0121 M and [NOCl] = 0.288 M. What is the molar concentration of NO(g) at equilibrium. (NO] 2.135 M 0.1022 M 0.01047 M 0.3636 M 0.00321 M At 900 degree C the equilibrium constant value (K_p) for the following reaction is measured at 3.05 times 10^-5. An equilibrium mixture was found to have the following partial pressure for CH_4. H_2S. and CS_2: P(CH_4) = 103 atm, P(H_2S)= 117 atm, and P(CS_2) = 88.5 atm. What is the partial pressure of H_2 gas at equilibrium. P(H_2) = atm? 243 atm 937 atm 589 atm 151 atm 61.2 atm A 5.75 L reaction vessel is filled with 0.515 moles of PCl_3 and 0.505 moles of Cb at 230 degree C. What are the molar concentrations of PCI_3, Cl_2, and PCl_5 at equilibrium?

Answer 1

0.61)-0444 4х. (o-23) (0 16.66 opcone P23 NO 。01리 lo3 (117) 2.- c" 5.223 x10 1? 2s) 4q Pcuso. 0126 M