2.A 1.035 L container (initially evacuated) is filled with 0.01032 moles of nitr

Question

2.A 1.035 L container (initially evacuated) is filled with 0.01032 moles of nitric oxide and 0.00430 moles of bromine gas. The two components react to form some NOBr. At equilibrium the total pressure is measured to be 235.2 torr at 323.15 K. Find KP and delta G* at this temperature. Assume ideal gas behavior. 2.A 1.035 L container (initially evacuated) is filled with 0.01032 moles of nitric oxide and 0.00430 moles of bromine gas. The two components react to form some NOBr. At equilibrium the total pressure is measured to be 235.2 torr at 323.15 K. Find KP and delta G* at this temperature. Assume ideal gas behavior.

Explanation / Answer

solution.

given,

volume= 1.035L

reaction

2NO + Br2 --------------> 2NOBr

initial moles 0.01032 0.00430 0

at equlibrium

(say x moles reacted) 2(0.01032-x) 0.00430-x 2x

total number of moles =[2(0.01032-x) + 0.00430-x + 2x]= n(say)

.

pressure at equilibrium 2(0.01032-x)/nP (0.00430-x)/nP P ................(1)

(using dalton's law,

let total pressure be P) P(no) P(br)

given P= 235.2 torr

Temperature = 323.15K

for NOBr,

PV=nRT

235.12*1.035 = x*62.363*323.15 (SINCE R= 62.363LTorrK?1??mol?1)

2x=0.012moles.

putting values in (1)

we get

p(no).

P(br).

substitute the values in the below formulas to get Kp and deltaG*

Kp= P^2/[P(no)^2*P(br)]

deltaG* = -RTln(Kp)

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