Posted by **sparkle** on Tuesday, October 5, 2010 at 2:41pm.

please help!

If the initial pressure of I2(g) is 1.738 atm, calculate the % decomposition of I2(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kp at 1000 K is 0.254. The initial pressure of the reaction products is 0 atm.

I2(g) = 2I(g)

- college chemistry -
**DrBob222**, Tuesday, October 5, 2010 at 2:46pm
Set up an ICE chart, substitute into Kp expression, and solve.

- college chemistry -
**sparkle**, Tuesday, October 5, 2010 at 2:54pm
i did.. it was wrong for the last time

- college chemistry -
**sparkle**, Tuesday, October 5, 2010 at 2:54pm
for the last time i did it*

- college chemistry -
**DrBob222**, Tuesday, October 5, 2010 at 2:58pm
If you post what you did perhaps I can find the error.

- college chemistry -
**sparkle**, Tuesday, October 5, 2010 at 5:28pm
initial:

I2 = 1.738 atm

2I = 0

change:

I2 = -2x

2I = x

equilibrium:

I2 = 1.738 - 2x

2I = x

so i set the equation as

0.254 = x/(1.738 - 2x)

and i solved for x. i got 0.292

and after that how do i get % decomposition?

- college chemistry -
**DrBob222**, Tuesday, October 5, 2010 at 6:00pm
equilibrium:

I^- (not 2I) = 2x

I2 = 1.738-x

Then Kp = pI^-^2/pI2

0.254 = (2x)^2/(1.738-x).

Solve for x. You didn't have 2x and then didn't square it.

%decomposition = (pI^-/1.738)*100 = ??

- college chemistry -
**daina soom**, Thursday, October 7, 2010 at 12:39am
What is the pressure in a 10.0- cylinder filled with 0.405 of nitrogen gas at a temperature of 327k?

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