# chemistry

posted by .

At 0.00 degrees C a 1.00 L flask contains 5.00 x 10^-2 mol N2, 1.50 x 10^2 mg O2, and NH3 at a concentration of 5.00 x 10^18 molecules/mL. What is the partial pressure of each gas, and what is the total pressure in the flask at atm?

• chemistry -

Convert mg and molecules to mols.
mols N2 you have.
mols O2 = grams/molar mass = ?
mols NH3 = #molecules/6.02E23 = ?

Use PV = nRT and solve for each pressure.
Then total P = sum of partial pressures.

• chemistry -

Thank you very much!

## Similar Questions

1. ### chem

Consider the decomposition of ammonium hydrogen sulfide: NH4Hs(s) <--> NH3(g) + H2S(g) In a sealed flask at 25*C are 10.0 g NH4HS, ammonia with a partial pressure of .692 atm, and H2S with a partial pressure of .0532 atm. When …
2. ### Chemistry

srry I placed the question in the wrong spot. The equation is 2NH3 <=> N2 + 3H2 1 mole of NH3 injected intoa 1L flask 0.3 moles of H2 was found the concentration of N2 at equlibrium is 0.1M how do I find the concentration of …
3. ### chemistry

A sample of NH4HS (s) is placed into a 2.65 L flask, containing 0.140 mols of NH3 (g). NH4++++>>nh3 (g) + h2s (g) KP = 0.108 wHAT will be the total gas pressure at 25 degrees in atm. I got about 1.361...i don't kno what im doing …
4. ### chemistry

A sample of NH4HS (s) is placed into a 2.65 L flask, containing 0.140 mols of NH3 (g). NH4++++>>nh3 (g) + h2s (g) KP = 0.108 wHAT will be the total gas pressure at 25 degrees in atm. I got about 1.361...i don't kno what im doing …
5. ### Chemistry

a tank contains a mixture of 3.0 mol of nitrogen gas, 2.0 mol of oxygen gas and 1.0 of carbon dioxide gas at 25 degrees celsius and a total pressure of 10.0 atm. Calculate the partial pressure in torr of each gas in the mixture?
6. ### chemistry

A tank contains a mixture of 3.0 mol of nitrogen 2.0 mol of oxygen and 1 mol of carbon dioxide at 25 degrees and a total pressure of 10 ATM calculate the partial pressure in torr of each gas?