Download the App!

Get 24/7 study help with the Numerade app for iOS and Android! Enter your email for an invite.

The equilibrium constant $\left(K_{P}\right)$ for the reaction$$\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)$$is 1.9 at $727^{\circ} \mathrm{C}$. What total pressure must be applied to the reacting system to obtain 0.012 mole of $\mathrm{CO}_{2}$ and 0.025 mole of $\mathrm{CO} ?$

Get the answer to your homework problem.

Try Numerade free for 7 days

Like

Report

$$1.3 \mathrm{atm}$$

Chemistry 102

Chapter 14

Chemical Equilibrium

Carleton College

Drexel University

Brown University

Lectures

10:03

In thermodynamics, a state of thermodynamic equilibrium is a state in which a system is in thermal equilibrium with its surroundings. A system in thermodynamic equilibrium is in thermal equilibrium, mechanical equilibrium, electrical equilibrium, and chemical equilibrium. A system is in equilibrium when it is in thermal equilibrium with its surroundings.

00:54

In chemistry, chemical equilibrium (also known as dynamic equilibrium) is a state of chemical stability in which the concentrations of the chemical substances do not change in the course of time due to their reaction with each other in a closed system. Chemical equilibrium is an example of dynamic equilibrium, a thermodynamic concept.

02:39

The equilibrium constant $…

02:43

At $700 .{ }^{\circ} \math…

01:08

01:22

04:20

02:37

Calculate the equilibrium …

01:00

An equilibrium is establis…

So for this question, we want to find the total pressure. And in order to find the total pressure where we don't already have it, we can look at using DK P equation because we know that partial pressure. It's just the mole fraction times the total of the products over the mole fraction times pressure total for the reactant. So first we want to find the mole fractions signified by a large uppercase X. Let's first start with air reactant. So we were told how many moles that we begin with and that is your a 0.12 And since we have only two, the gaseous form, we're only going take into account those two always who used in the KP or equilibrium, concentration, equilibrium, constant equation in regards to partial pressure that we're gonna add harbor monoxide. They were going to do this the same thing for this one, with its values to your 0.0 to 5 and then the total. So we calculate this out. We find mole fraction of carbon dioxide is 0.32 in the more fraction of her pin bun oxide is 0.68 I don't know why it did that they're real. And then we can plug this into our KP equation, so we know that is gonna equal total pressure. Times 0.68 Now we're gonna raise it to the power of to do, to destroy geometry here. Ready? All this over total pressure times. This is a reactant on the bottom. And then retreat the total pressure like we would any other X value, like we were solving for X. And we find that the total pressure this problem is 1.3 a. T. M.

View More Answers From This Book

Find Another Textbook

Numerade Educator