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Enter your answer in the provided box. Given the same reactant concentrations, the reaction CO(g) +...
13.38 Given the same reactant concentrations, the reaction CO(g) + Cl2(g) — COC12(8) at 250°C is 1.50 x 10 times as fast as the same reac- tion at 150°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
Given the same reactant concentrations, the reaction CO(g) + Cl_2(g) rightarrow COCl_2(g) at 263 degree C is 219 times as fast as the same reaction at 153 degree C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g) ΔH =-184.6 kJ/mol If 5.0 moles of H2 reacts with 5.0 moles of C12 to form HC1 at 1.0 atm, what is Δ U for this reaction? Assume the reaction goes to completion and Δ V= 0 L (The conversion factor is 1 L·atm = 101.3 J.) kJ
Enter your answer in the provided box. Assume that a reaction takes place at 340 K and 380 K. What must the activation energy be for the rate constant to double over this temperature range? 0 kJ/mol
Enter your answer in the provided box. The rate constant of a first-order reaction is 2.35 x 10-45-1 at 350.°C. If the activation energy is 135 kJ/mol, calculate the temperature at which its rate constant is 9.00 x 10-45-1. °c
9.Enter your answer in the provided box. S(rhombic) + O2(g) → SO2(g) ΔHo rxn= −296.06 kJ/mol S(monoclinic) + O2(g) → SO2(g) ΔHo rxn= −296.36 kJ/mol calculate the enthalpy change for the transformation S(rhombic) → S(monoclinic) (Monoclinic and rhombic are different allotropic forms of elemental sulfur.) _______kJ/mol 10. Enter your answer in the provided box Use the following data to calculate ΔHo/f for CS2(l): C(graphite) + O2(g) → CO2(g) ΔHo rxn= −393.5 kJ/mol S(rhombic) + O2(g) → SO2(g) ΔHo rxn=...
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.325 moles of CO and 0.325 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.355 moles of CO and 0.355 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) goes to COCl2(g) . Calculate the equilibrium concentrations of reactant and products when 0.320 moles of CO and 0.320 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = ___M [Cl2] = ___M [COCl2] = ___M
Enter your answer in the provided box. In the Mond process for the purification of nickel, carbon monoxide is reacted with heated nickel to produce Ni(CO), which is a gas and can therefore be separated from solid impurities: Ni(s) + 4C0g)#Ni(CO),g) Given that the standard free energies of formation of CO(g) and Ni(CO),(g) are -137.3 and -587.4 kJ/mol, respectively, calculate the equilibrium constant of the reaction at 56.0°C. Assume that AG is temperature-independent.