This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Write the balanced chemical equation and the equilibrium constant expression (K_c). The reaction is: CO(g) + Cl_2(g) COCl_2(g) The equilibrium constant expression in terms of concentrations is: K_c = [COCl_2][CO][Cl_2] Step 2: Substitute the given equilibrium concentrations into the K_c expression and calculate K_c. Given concentrations: [CO] = 0.623 M [Cl_2] = 0.068 M [COCl_2] = 0.25 M K_c = 0.25 M(0.623 M)(0.068 M) K_c = (0.25)/(0.042364) K_c ≈ 5.899 The units for K_c are MM · M = M^-1 or L/mol. K_c = 5.90 L/mol Step 3: Calculate the change in the number of moles of gas ( n). n = (moles of gaseous products) - (moles of gaseous reactants) From the balanced equation: Moles of gaseous products = 1 (for COCl_2) Moles of gaseous reactants = 1 (for CO) + 1 (for Cl_2) = 2 n = 1 - 2 = -1 Step 4: Convert the temperature to Kelvin. Given temperature T = 75^. T(K) = 75 + 273.15 = 348.15 K Step 5: Calculate K_p using the relationship K_p = K_c(RT)^ n. Given R = 0.0821 atm K^-1 mol^-1. K_p = K_c(RT)^ n K_p = (5.899 L/mol) ( (0.0821 atm K^-1 mol^-1)(348.15 K) )^-1 K_p = (5.899 L/mol) ( 28.580315 atm L mol^-1 )^-1 K_p = (5.899 L/mol) ( (1)/(28.580315 atm L mol)^-1 ) K_p = (5.899 L/mol) (0.034989 atm^-1 L^-1 mol) K_p ≈ 0.2064 atm^-1 K_p = 0.206 atm^-1