Question

In: Chemistry

A) What is the Hrxno in (kJ) for the reaction below, given the relevant table on...

A) What is the H_rxn^o in (kJ) for the reaction below, given the relevant table on the info sheet. PbO(s) + 2HBr(g) ---> PbBr₂(s)+H₂O(g).

a) -273

b) -229

c) -265

d) Not enough information provided.

B. What is the H_rxn^o in (kJ) for 2PbBr₂(s) + 2H₂O(g) ---> 2PbO(s) +4HBr(g) using the thermochemical equation in part A.

a) 545

b) 530

c) 458

d) 229

Expert Solution

PbO(s) + 2HBr(g) ---> PbBr₂(s)+H₂O(g).

Hrxn = H⁰f products - H⁰f reactants

= -241.818-278.9 -(-218.99+ 2*-36.4)

= -229KJ/mole

b. -229

B. 2PbBr₂(s) + 2H₂O(g) ---> 2PbO(s) +4HBr(g)

Hrxn = H⁰f products - H⁰f reactants

= 4*-36.4+ 2*-218.99-(-2*278.9 + 2*-241.818)

= 458KJ/mole

Or

PbBr₂(s) + H₂O(g) ---> PbO(s) +2HBr(g) Hrxn = 229Kj/mole

2PbBr₂(s) + 2H₂O(g) ---> 2PbO(s) +4HBr(g) Hrxn = 2*229 = 458Kj/mole

c) 458 >>>>answer

queen_honey_blossom answered 1 year ago

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