At 1261 degrees Celsius the equilibrium constant for the reaction: 2 IBr(g) —><— I2(g) + Br2(g)
is Kp= 1.09. If the initial pressure of IBr is 0.00985 atm, what are the equilibrium partial pressures of IBr, I2, and Br2?
1) p(IBr) = ___
2) p(I2) = ____
3) p(Br2) = ____
Moles of IBr= 2
Moles of I2 = 1
Volume = 67.2 L
Temperature = 273 + 1261 = 1534 K
PV = nRT
Partial pressure of IBR = 2×0.0821×208/67.2= 0.508atm
Partial pressure of I2= 1×0.0821×208/67.2= 0.254atm
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