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10 Nov 2019
For the reaction 2 HBr(g) + Cl2(g) rightarrow 2 HCl(g) + Br2(g) Write the equilibrium constant expression for the reaction. Using the following G degree values, calculate delta6degree for the reaction. HBr(g) = -53.22 kJ/mol HCl(g)= -95.27 kJ/mol Cl2(g)= 0 kJ/mol Br2(g)=3.14 kJ/mol Calculate the equilibrium constant Keq be at 298 K. Does this equilibrium lie more with reactants or products?
For the reaction 2 HBr(g) + Cl2(g) rightarrow 2 HCl(g) + Br2(g) Write the equilibrium constant expression for the reaction. Using the following G degree values, calculate delta6degree for the reaction. HBr(g) = -53.22 kJ/mol HCl(g)= -95.27 kJ/mol Cl2(g)= 0 kJ/mol Br2(g)=3.14 kJ/mol Calculate the equilibrium constant Keq be at 298 K. Does this equilibrium lie more with reactants or products?
Irving HeathcoteLv2
20 Aug 2019