Question

a chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature:

$$\\ce{n_{2}(g) + 3h_{2}(g)\ ightleftharpoons 2nh_{3}(g)}$$

$$k_{p}=2.\times 10^{-6}$$

he fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 4.4 atm of hydrogen gas. use this data to answer the questions in the table below.

can you predict the equilibrium pressure of $$\ce{nh_{3}}$$, using only the tools available to you within aleks? yes no

if you said yes, then enter the equilibrium pressure of $$\ce{nh_{3}}$$ at right. atm round your answer to 1 significant digit.

Explanation:

Step1: Write the expression for \(K_p\)

For the reaction \(N_2(g)+3H_2(g)
ightleftharpoons 2NH_3(g)\), the equilibrium constant expression is \(K_p=\frac{P_{NH_3}^2}{P_{N_2}\times P_{H_2}^3}\).

Step2: Analyze the magnitude of \(K_p\)

Given \(K_p = 2\times10^{-6}\), which is a very small value. This indicates that the equilibrium lies far to the left (reactant - favored). The change in the partial pressures of \(N_2\) and \(H_2\) to form \(NH_3\) is negligible. So, we can assume that \(P_{N_2}\approx6.0\ atm\) and \(P_{H_2}\approx4.4\ atm\) at equilibrium.

Step3: Solve for \(P_{NH_3}\)

Substitute the values into the \(K_p\) expression:

$$
LATEXBLOCK0
$$

Answer:

yes, \(0.03\ atm\)