Consider the following elementary reaction: CFC13(g)-CFC12(9)+Clg) Suppose we let k1 stand for the rate constant of this reaction, and k1 stand for the rate constant of the reverse reaction Write an expression that gives the equilibrium concentration of Cl in terms of k, k_1, and the equilibrium concentrations of CFCI3 and CFCI2 1. K-1 [ci]

Be sure to answer all parts. the following equilibrium constants were determined at 1123 k: c(s) + co2(g) ⇌ 2co(g) k'p = 1.30 × 1014 co(g) + cl2(g) ⇌ cocl2(g) k''p = 6.00 × 10−3 calculate the equilibrium constant at 1123 k for the reaction: c(s) + co2(g) + 2cl2(g) ⇌ 2cocl2(g) 4.68 × 10 9 (enter your answer in scientific notation.) write the equilibrium constant expression, kp: