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).
Expert's answer

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

Comments

No comments. Be first!

Leave a comment

Ask Your question

LATEST TUTORIALS
New on Blog
APPROVED BY CLIENTS
paypal