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# ideal gas law question watch

1. i don't understand how to do this question

A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47 oC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.
2. (Original post by qatarownz)
i don't understand how to do this question

A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47 oC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.
Do you know the definition of partial pressure?
3. (Original post by charco)
Do you know the definition of partial pressure?
it means the total pressure when summed together
4. (Original post by qatarownz)
i don't understand how to do this question

A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47 oC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.
By using this law .. You have the volume , mass and temrature . find number of moles from the mass then you can culculate partial pressure .
The total pressure is the sum of partial pressure of gases in mixture .
5. this what I got

Moles of CO= 8.8 g/28.008 g/mol= 0.314
Moles of H2= 2 g/2.0156 g/mol= 0.992

P(CO)= nRT/V = [(0.314)(0.08206)(47+273.15)]/5.0= 1.65 atm

P(H2)= nRT/V = [(0.992)(0.08206)(47+273.15)]/5.0= 5.21 atm

Partial Pressure of H2 = 0.992/(0.314+ 0.992) = 0.76

0.76*5.21 = 3.96 atm

Pressure Total = 1.65 + 5.21 = 6.86 atm

6. (Original post by qatarownz)
this what I got

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I think its correct
7. (Original post by qatarownz)
this what I got
A 5.0 L container is filled with 8.8 g of CO(g) and 2.00 g of H2(g). The temperature is 47ºC. Calculate the partial pressure of H2 and the total pressure of the gas mixture.

The partial pressure of a gas is the pressure that it would exert if it were on its own.
It can be calculated by the mole fraction x the total pressure.

So deal with each gas on its own:

CO(g) 8.8g = 8.8/28 mol = 0.314

P = nRT/V = 0.314 x 8.314 x 320/5 = 167.2 kPa

H2(g, 2g = 2/2 mol = 1 mol

P = nRT/V =1 x 8.314 x 320/5 = 532.1 kPa

Total pressure = 699.3 kPa

If you want the answer in atmospheres divide by 101.3 = 6.90 atm

You are correct (the slight difference results from my use of rounded Mr values)

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