Asked by KL

At o degrees celcius, a 1.0-L flask contains 5.0 x 10^-2 mol N2, 1.5 x 10^2 mg O2 and 5.0 x 10^21 molecules of NH3. What is the p00artial pressure of each gasnand what is the total pressure in the flask?
I need to understand how to calculate it, formula and how to get the proper answer..please!
Answered by DrBob222
Note the correct spelling of celsius. Do you want my help or would you prefer to wait on another tutor?
Answered by KL
I want your help providing you explan it nand show me hoe=w to gt the aswers so ai undrerahf i!
Answered by Ms. Sue
It's hard for me to take you seriously, KL. You have seven spelling/typo errors in your last response. My conclusion is that you really don't care.
Answered by DrBob222
This is not a complicated problem but it is long and involves several steps.
1. Convert the gases to mols.
a. you have mols N2 as 0.05.
b. Convert 150 mg O2 to grams, then mols = grams/molar mass. mols O2 = ?
c. Convert 5E21 molecules NH3 to mols. That is 5E21 molecules x (1 mol/6.02E23 molecules) = ? mols NH3.

2. Find individual pressure of each gas. Use PV =nRT. Substitute n for each gas. You know R and T (remember T must be in kelvin), P is in atm and volume in L.

3.. Now find the total pressue by adding the partial pressures of each gas. The sum is Ptotal.
Post your work if you have trouble so I will know where you are going wrong.
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