Recent content by blackjack18

A sealed balloon is filled with 1.00 L of He gas at 23 deg C and 1.00 atm. The balloon rises to a point in the atmosphere where the pressure is 220 torr and the temperature is -31 deg C. What is the final volume of the balloon after it reaches an altitude where the pressure is 220 torr? If...

A mixture of 1.00 g of H2 and 1.00 g of He is placed in a balloon of volume 1.0 L when filled with these gases at 27 deg C. A) calculate the partial pressure of each gas and the total pressure pressure of H2-12.315 atm? pressure of He-6.158 atm? B) calculate the mole fraction...

775=0.5(constant)(298), then divided by 775

yes, is that the answer to the following: What is the volume of an ideal gas at 1 atm, 12 L, and 25 degrees Celsius if the pressure is decreased to 0.8 atm at 25 degrees Celsius?

ok, I am not sure about this, but is the answer 1.59?

what is the constant? or is there one? if so, how do i determine what it is?

yes, is that the answer to the following: What is the volume of an ideal gas at 1 atm, 12 L, and 25 degrees Celsius if the pressure is decreased to 0.8 atm at 25 degrees Celsius?

what volume is occupied by 2.0 g of He at 25 degrees C and a pressure of 775 mm?

is the answer v2=15 L?

Should Boyle's Law be used in this problem, since the temperature remains constant: What is the volume of an ideal gas at 1 atm, 12 L, and 25 degrees Celsius if the pressure is decreased to 0.8 atm at 25 degrees Celsius?

alrighty, thanks...

is 44.8 L/mol is the answer?

i don't know...boyles law states P x V = constant...and i don't know what the pressure is

all i really need help with is the pressure... i have the formula for the problem i think (boyle's law) but i do not know the what the pressure is...

If 0.5 mol of nitrigen gas occupies a volume of 11.2 L at 0 degrees Celsius, what volume will 2 mol of nitrogen gas occupy at the same temperature and pressure?