A chemist is studying the following equilibirum, which has...

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2(g) + 3 H2(g) ? 2 NH3(g) Kp = 1. x 10^-1 He fills a reaction vessel at this temperature with 7.0 atm of nitrogen gas and 5.4 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the tools available to you within ALEKS? yes no If you said yes, then enter the equilibrium pressure of NH3 at right. Round your answer to 1 significant digit. atm

Transcript

00:01 The equilibrium reaction is n2 reacting with 3h2 to produce 2nh3, and they tell us at a particular temperature that kp is equal to 0 .1.

00:20 If we know that the reaction vessel is filled at this temperature with 7 atmospheres of nitrogen, 7 .0 and 5 .4 atmospheres of hydrogen, then can we predict the equilibrium pressure of nh3? and the answer to that is yes, otherwise there wouldn't be a question to answer.

00:52 So if we said yes, what is the equilibrium pressure? pressure, but without any ammonia to begin with, then this is going to shift to the right to create ammonia, decreasing the pressure of nitrogen by x and the pressure of hydrogen by 3x, and will increase the pressure of ammonia by 2x.

01:16 So we'll have at equilibrium 7 .0 minus x, 5 .4 minus 3x, and 2x.

01:26 So our kp, 0 .10, is going to be equal to the pressure of our product, ammonia, 2x, raised to its coefficient of 2 divided by the pressure of the reactant nitrogen 7 .0 minus x and the pressure of h2 5 .4 minus 3x and then we cube that with our kp value being neither very large nor small we can't drop these x values we we need to retain them.

02:08 So that means we're going to have to solve this very complicated algebraic expression.

02:14 So i'm hoping that your instructor allows you to use a calculator or a solver program.

02:19 I let my students use a calculator, so i'll use a calculator to solve for x.

02:24 We can estimate that with this being around 1, that we'll have about equal amounts of all of them.

02:33 That term equal is relative but we could probably assume that each of these this is probably going to decrease by maybe half its value at 3 .5 so we could estimate x to be about 3 .5 and that'll help us solve using a solver program and and estimating 3 .5, we end up getting x equal to 5 .08 atmospheres.

03:02 So now we can determine what the ammonia concentration is...

Question

Please give Ace some feedback