Consider the reaction 2nog o2g rightleftharpoons 2no2g part...

Consider the reaction: $$2NO(g) + O_2(g) \rightleftharpoons 2NO_2(g)$$ Part A A reaction mixture at 175 K initially contains 522 torr of NO and 421 torr of $$O_2$$. At equilibrium, the total pressure in the reaction mixture is 748 torr. Calculate $$K_p$$ at this temperature. Express your answer to three significant figures. $$K_p = 29.4$$ Part B A second reaction mixture at 175 K initially contains 365 torr of NO and 215 torr of $$O_2$$. What is the equilibrium partial pressure of $$NO_2$$ in this mixture? Express your answer in torr to three significant figures. $$P_{NO_2} = $$ torr

Transcript

00:04 For a, let's calculate the kp value.

00:09 Start by creating an ice table.

00:21 And we'll fill in what we have.

00:24 We'll do this ice table in tor.

00:29 We have 522 tour initially.

00:36 And 421 tor, 421 tor.

00:38 4 .0.

00:42 Let's tell you it would shift to the right like so.

00:52 Plate our ice table we are told that the total pressure of the system at equilibrium is equal to 748 so let's calculate or let's use that next so the total pressure at equilibrium would be the partial pressure of n0 plus the partial pressure of o2 plus the partial pressure of n02 we're told that that's equal to 748 is equal to 522 minus 2x plus 421 minus x plus 2x.

01:48 Solving this for x will yield of 195.

01:57 Therefore, the partial pressure of no at equilibrium, we don't.

02:10 Minus 522 minus 2x and this would be equal to 132 tour the partial pressure of 02 at equilibrium would be equal to 421 minus x and this would be equal to 226 torr and the partial pressure of n02 at equilibrium would be equal to 2 times x and therefore this would be equal to 390 tor.

02:58 Now these are all our partial pressures in equilibrium.

03:01 We'd have to convert these two atmospheres.

03:06 So let's go ahead and do that.

03:09 760 tor, one atmosphere.

03:17 This would be equal to 0 .174 atmospheres.

03:22 0 .297 atmospheres and 0 .513 atmospheres.

03:56 Using these values, let's calculate our equilibrium constant.

04:00 Let's first define our equilibrium constant, which will be equal to the partial pressure of no2 squared over the partial pressure of no squared times a partial pressure of o2 in the denominator.

04:15 Let's plug in our values.

04:18 0 .513 squared divided by 0 .174 squared .297.

04:29 Let's solve for equilibrium constant.

04:41 And this works out to an equilibrium constant is equal to 29 .3...

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