- #1

- 3

- 0

You are using an out of date browser. It may not display this or other websites correctly.

You should upgrade or use an alternative browser.

You should upgrade or use an alternative browser.

- Thread starter poopflinger15
- Start date

- #1

- 3

- 0

- #2

- 650

- 1

[tex]n_1*M + 2n_2*M = 2.3 g [/tex]

Where

n

n

M : Molecular mass of NO

Also PV=(n1+n2)RT

So u have two unknown and two equations u can find n1 & n2 from it And Hence Kp or partial pressure

- #3

GCT

Science Advisor

Homework Helper

- 1,728

- 0

Using PV=nRT, since you know P and T, you can solve for the solution in the form of moles per liter. For the rest of the problem we will assume a volume of one liter (it does not matter either way since it is only a matter of proportion). Since you have the grams pertaining to this situation you essentially have the "average molar mass of this situation." That is 2.3 grams/the total number of moles (which you are to figure out).

[molar mass of the nitrogen compound (grams/moles) X N1 (number of nitrogen compound)] + [molar mass of the dinitrogen compound (grams/moles) X N2 (number of the dinitrogen compound)]

all of this divided by 2

Solve for the proportion N1/N2, that is proportional to the moles.

Notice however, that the Kp equation for the reaction pertaining to the addition of the nitrogen to form the dinitrogen should have an exponent of 2 on the pressure of the nitrogen compound; we know that according to the stochiometric equation that there are two moles of the nitrogen compound for every dinitrogen compound.:

Kp = [partial pressure of dinitrogen compound p]/[partial pressure of nitrogen compound]^2

Note also that you will need to convert moles into pressure because of the presence of an exponent (with the assumption of 1 L as the volume, volume is insignificant information in this problem).

--------------

Online help with college and high school chemistry

http://groups.msn.com/GeneralChemistryHomework [Broken]

[molar mass of the nitrogen compound (grams/moles) X N1 (number of nitrogen compound)] + [molar mass of the dinitrogen compound (grams/moles) X N2 (number of the dinitrogen compound)]

all of this divided by 2

Solve for the proportion N1/N2, that is proportional to the moles.

Notice however, that the Kp equation for the reaction pertaining to the addition of the nitrogen to form the dinitrogen should have an exponent of 2 on the pressure of the nitrogen compound; we know that according to the stochiometric equation that there are two moles of the nitrogen compound for every dinitrogen compound.:

Kp = [partial pressure of dinitrogen compound p]/[partial pressure of nitrogen compound]^2

Note also that you will need to convert moles into pressure because of the presence of an exponent (with the assumption of 1 L as the volume, volume is insignificant information in this problem).

--------------

Online help with college and high school chemistry

http://groups.msn.com/GeneralChemistryHomework [Broken]

Last edited by a moderator:

- #4

- 210

- 0

There's nothing quite like a lungful of NO2 in the morning. It really gives your day a kick.

Share: