# Chemistry-Gases

posted by .

A mixture of gases is prepared from 76.9 g of O2 and 16.0 g of H2. After the reaction of O2 and H2 is complete, what is the total pressure of the mixture if its temperature is 178 ÂșC and its volume is 11.0 L? What are the partial pressures of the gases remaining in the mixture?

• Chemistry-Gases -

2H2 + O2 ==> 2H2O
mols H2 = grams/molar mass = about 8 but you need to calculate that as well as all of the other values that follow.
mols O2 = about 4.8. What is the limiting reagent? I think that's H2 and it will produce about 8 mols H2O.
How much O2 will be used. That's
8mols H2 x (1 mol O2/2 mol H2) = 8 x (1/2) = 4 so you will have 0.8 mols O2 remaining. Summary. We have no H2 left, 0.8 mols O2, and we have formed 8 mols H2O. Add total mols and substitute into PV = nRT and solve for Ptotal.

Then calculate mole fraction O2 and H2O.
Then pO2 = XO2 x Ptotal
pH2O = XH2O x Ptotal.

## Similar Questions

1. ### Chemsitry II

mole fraction is equal to partial pressure divided by the total pressure Total pressure= sum of partial pressure use PV=nRT where n= number of moles equation become PV/RT=n make sure to convert the temperature to Kelvin and to use …
2. ### chemistry

The gases in a mixture have the following partial pressures at the same volume and temperature: 1,013,000 Pa nitrogen, 700. mmHg argon, 1.20 atm of helium, 790. torr oxygen, and 0.50 atm of carbon dioxide. What is the total pressure …
3. ### Chemistry

What pressure will be exerted by each of the gases in the following mixture if the total pressure of the mixture amounts to 768.8 torr?
4. ### chemistry

a mixture of methane and ethane is stored in a container at 294 mmHg. The gases are burned in air to form co2 and h2o. if the pressure of co2 is 357 mmhg measured at the same temperature and volume as the original mixture, calculate …
5. ### chemistry

Suppose a mixture containing 3.52 g H2 and 37.0 g NO has a total pressure of 2.21 atm. What are the partial pressures of both gases in the mixture?
6. ### Chemistry

A 1.0 liter flask is filled with a mixture of two gases at 20. oC until a pressure of 14.43 atm is established. If 0.40 grams of the mixture is hydrogen, how many moles are there of the other gases?
7. ### Chemistry

Consider the following reaction: 4NH3(g) +5O2(g) -->4NO(g) +6H2O(g) Suppose we have two flasks connected by a stopcock. In one flask, we have 2.0L of NH3(g) at a pressure of .500 atm. In the other flask, we have 1.00L of O2(g) at …
8. ### chemistry

A mixture of gases has the following partial pressure for the component gases at 20 degrees Celsius: oxygen 180.0 torr, nitrogen 3200 torr, and hydrogen 246.0 torr. Calculate the pressure of the mixture.
9. ### Chemistry

In an experiment, a mixture of two gases occupies a volume of 3.00 L at a temperature of 22.5 degree centigrade. The mixture contains 14.0 g of water, 11.5 g of oxygen, and 37.3 g of nitrogen. Calculate the total pressure and the partial …
10. ### Chemistry

A mixture of gases contains 2.41 moles of O2, 1.24 moles of H2 and 1.92 moles of C. Calculate the partial pressure of gases if the total pressure is 3.0 atm

More Similar Questions