# Answer to Question #55559 in Other Chemistry for Mariam

Question #55559

The reaction between phosphorous,P4(s), and chlorine, Cl2(g), is exothermic and leads to either PCl3(g) or PCl5(g) depending on the stoichiometric amount of Cl2(g) used. Given the following two chemical equations (EQ 1 and EQ 2) and their associated enthalpy changes for the formation of PCl3(g) and PCl5(g);

EQ 1: P4(s) + 6Cl2(g) → 4PCl3(g) = -2439 kJ/mol-rxn

EQ 2: P4(s) + 10Cl2(g) → 4PCl5(g) = -3438 kJ/mol-rxn

EQ 3: PCl5(g) → PCl3(g) + Cl2(g) = ?

a. Calculate the expected enthalpy change for the decomposition of one mole of PCl5(g) shown in equation 3 (EQ 3).

b. Calculate the expected enthalpy change for the decomposition of 10.50 g of PCl5(g) shown in equation 3 (EQ 3).

EQ 1: P4(s) + 6Cl2(g) → 4PCl3(g) = -2439 kJ/mol-rxn

EQ 2: P4(s) + 10Cl2(g) → 4PCl5(g) = -3438 kJ/mol-rxn

EQ 3: PCl5(g) → PCl3(g) + Cl2(g) = ?

a. Calculate the expected enthalpy change for the decomposition of one mole of PCl5(g) shown in equation 3 (EQ 3).

b. Calculate the expected enthalpy change for the decomposition of 10.50 g of PCl5(g) shown in equation 3 (EQ 3).

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