chem

posted by .

Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide.
H2(g) + CO2(g) --> H2O(g) + CO(g)

(a) Laboratory measurements at 986°C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 1.0 L container. Calculate the equilibrium constant for the reaction at 986°C.

I got 2.1e2. I did (.11)(.11)/(.087)(.087)

What are i doing wrong?

(b) Suppose 0.052 mol each of H2 and CO2 are placed in a 1.5 L container. When equilibrium is achieved at 986°C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of K calculated in part (a).]

[CO]
______ mol
[H2O]
______ mol

• chem -

The numbers you have for Keq are correct; I assume you are punching the wrong buttons on your calculator. For (0.11)^2/(0.087)^2 I get 1.6

For part b.
0.052moles/1.5L = 0.0347M
..............H2 + CO2 ==> H2O + CO
initial...0.0347..0.0347.....0.....0
change......-x......-x.......+x....+x
equil...0.0347-x..0.0347-x....x.....x
Substitute into Ka expression and solve for x. The question asks for moles; therefore, x is molarity and M x L = moles.
Post your work if you get stuck.

• chem -

thanks

Would you get the same answer for both parts of b?

• chem -

Since you started with the same molarity for each and you used x of each, then the moles of each will be the same at equilibrium.

• chem -

ok so I did (x)(x)/(.03466)(.03466)= 1.6. I solved for x and got .0438. Do I have to do anything with this number to get the correct answer?
Can you check my work?

Thanks:)

• chem -

I would have rounded the 0.034666 to 0.03467 (and that's too many significant figures). However, it's (x)(x)/(0.03467-x)^2. What did you do with the -x in the 0.03467 - x term? Throw it away. You can't do that (at least not in this problem). You must solve the quadratic. I don't get anything like 0.0438M for an answer. After you find the M for x, you must subtract it from 0.03467 to find (CO2) and (H2), then multiply (CO2), (H2), (H2O), and (CO) by 1.5 to obtain moles (since the problem asks for each of these in moles.)

• chem -

Sorry I am soo confused right now O.O. is there anyway u can explain this in simplier form?

Respond to this Question

 First Name School Subject Your Answer

Similar Questions

1. chemistry

how do I write a balanced equation showing aqueous hydrogen carbonate, to give liquid water and carbon dioxide gas H2O(l) + CO2(g) ==>H2CO3(aq) to show the formation of dihydrogen carbonate (carbonic acid). To show the decomposition …
2. chemistry

If 1.00 mol each of carbon dioxide and hydrogen is initially injected into a 10.0-L reaction chamber at 986 degrees Celsius, what would be the concentrations of each entity at equilibrium?
3. chemistry

I would also like to see Nathaniels work solved:P I have a similar question If 1.00 mol each of carbon dioxide and hydrogen is initially injected into a 10.0-L reaction chamber at 986 degrees Celsius, what would be the concentrations …
4. Chemistry

Assuming all volume measurements are made at the same temperature and pressure, how many liters of carbon dioxide gas can be produced when 12.8 liters of oxygen gas react with excess carbon monoxide?
5. Chemistry

Toxic Carbon monoxide gas is produced when fossil fuels such as gasoline, burn wihtout sufficient oxygen gas. The CO ca eventually be converted to CO2 inthe atmsphere. Automobie cata;yctic converters are desgned to speed up this conversion: …
6. Chem (repost)

Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) --> H2O(g) + CO(g) (b) Suppose 0.052 mol each of H2 and CO2 are placed in a 1.5 L container. When equilibrium is achieved …
7. Chemistry

An equilibrium mixture contains 0.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) + H2O(g) <-> CO2(g)+ H2(g) …
8. chemistry

1-Dinitrogen tetroxide (N2O4) dissociates according to the equation: N2O4 ⇌ 2NO2 An equilibrium reaction mixture at 25 ºC was found to have the partial pressure of N2O4 as 72 kPa whilst the partial pressure of nitrogen dioxide …
9. chemistry help

When carbon dioxide and carbon react the balanced equation is Co2+C--------------2Cq Calculate the mass of carbon monoxide formed from 4.4g of carbon dioxide
10. CHEMISTRY PLEASE HELP APPRECIATE IT LOTS!

7.) How many moles of fluroine are required to react with 12 g of sodium iodide?

More Similar Questions

Post a New Question