Question

Assuming that only the listed gases are present, what would be the mole fraction of oxygen gas be for each of the following situations? A.) A balloon which contains 4.53 g of nitrogen and 3.61 g of oxygen. B.) A gas sample of 2.31 atm of oxygen gas and 3.75 atm of hydrogen gas that react to form water vapor. Assume the volume of the container and the temperature inside the container does not change. A.) A sample of gas contains 6.43 moles at 37.8 °C in a volume of 3.61 L. At what pressure is this gas, in atm? B.) A sample of gas contains 6.43 moles at 37.8 °C in a volume of 3.61 L. If 2.67 moles of gas are added, what is the new volume (in L) assuming temperature and pressure do not change. C.) A sample of gas contains 6.43 moles at 37.8 °C in a volume of 3.61 L. If 0.530 moles of gas are removed from the initial 6.43 moles and the temperature increased to 52.8 °C while pressure is held constant, then what is the new volume of the gas, in liters? A.) A sample of helium is initially at 675 torr in a volume of 2.85 L. If this sample of helium is at 24.7 °C, then how many moles of helium are present? b.) What is the density of this gas sample 24.7 C, in g/L. c) Suppose instead of helium you had a sample of argon gas at 24.7 C. How many moles of argon would be present with the same pressure and volume? d.) What would be the density of the argon gas sample at 24.7 C, in g/L. e.) Which one of the following best explains why the densities are different?

          Assuming that only the listed gases are present, what would be the mole fraction of oxygen gas be for each of the following situations?
A.) A balloon which contains 4.53 g of nitrogen and 3.61 g of oxygen.
B.) A gas sample of 2.31 atm of oxygen gas and 3.75 atm of hydrogen gas that react to form water vapor. Assume the volume of the container and the temperature inside the container does not change.

A.) A sample of gas contains 6.43 moles at 37.8 °C in a volume of 3.61 L. At what pressure is this gas, in atm?
B.) A sample of gas contains 6.43 moles at 37.8 °C in a volume of 3.61 L. If 2.67 moles of gas are added, what is the new volume (in L) assuming temperature and pressure do not change.
C.) A sample of gas contains 6.43 moles at 37.8 °C in a volume of 3.61 L. If 0.530 moles of gas are removed from the initial 6.43 moles and the temperature increased to 52.8 °C while pressure is held constant, then what is the new volume of the gas, in liters?

A.) A sample of helium is initially at 675 torr in a volume of 2.85 L. If this sample of helium is at 24.7 °C, then how many moles of helium are present?
b.) What is the density of this gas sample 24.7 C, in g/L.
c) Suppose instead of helium you had a sample of argon gas at 24.7 C. How many moles of argon would be present with the same pressure and volume?
d.) What would be the density of the argon gas sample at 24.7 C, in g/L.
e.) Which one of the following best explains why the densities are different?

Added by Justin M.

Question

Please give Ace some feedback