Am also having trouble with these problems and i need to knowhow to do them plea

Question

Am also having trouble with these problems and i need to knowhow to do them please explain to me every step thank you!! 1.A mixture of gases contains 2.40 gof N2, 4.61 g of H2,and 8.15 g of NH3. If the totalpressure of the mixture is 2.27 atm, whatis the partial pressure of each component?
PN2 _________atm
PH2 _________ atm
PNH3 ________ atm
2. (a) Calculate the density of NO2 gas at0.954 atm and 33°C.
answer in________ g/L

(b) Calculate the molar mass of a gas if 3.30 g occupies 0.866 L at695 torr and 35°C.
answerin__________ g/mol

Am also having trouble with these problems and i need to knowhow to do them please explain to me every step thank you!! 1.A mixture of gases contains 2.40 gof N2, 4.61 g of H2,and 8.15 g of NH3. If the totalpressure of the mixture is 2.27 atm, whatis the partial pressure of each component?
PN2 _________atm
PH2 _________ atm
PNH3 ________ atm
2. (a) Calculate the density of NO2 gas at0.954 atm and 33°C.
answer in________ g/L

(b) Calculate the molar mass of a gas if 3.30 g occupies 0.866 L at695 torr and 35°C.
answerin__________ g/mol

Explanation / Answer

For part 1: 1) Find the number of moles of each gas (divide the grams by the MWof the compound) 2) Find the mol fraction of each gas (mols of one gas over thetotal mols) 3) Find the partial pressure using the formula P1 =X1*Ptot where X is the mol fraction) 2a) Rearrange the ideal gas formula. n/V = P/(RT). Solve for n/V and watch your units. After that, multiply bythe MW of NO2 to get the density. 2b) Rearrange the ideal gas formula to solve for the moles,n. Then take the grams you started with divided by the molsto get the MW. Hope that helps Be sure to watch your units, especially for the gas constant.

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