Chemisty Question - Edit 1
Before modification by Hobo at 09/05/2011 06:46:47 PM
So we were given this question forever ago in my class, and he said we would go over it on a later day in class, but whether he forgot or I wasn't there I never saw the answer to it. And now, school is over for the summer so I can't ask him, but it's been bugging me, so hopefully someone here will know what to do.
A series of measurements are made in order to determine the molar mass of an unknown gas. First, a flask is evacuated and found to weigh 134.567 g. It is then filled with the gas to a pressure of 735 mm Hg at 31 degrees C and found to weigh 1067.9 g. (The density of the water at this temperature is 0.997 g/ml.) Assuming that the ideal-gas equation applies, calculate the molar mass of the unknown gas.
Yeah, I've looked at this for a while and can't really see what to do, I swear it doesn't give enough information. And then it says "the" water, a definite article instead of using "some" (or not using an article at all) the indefinite article, but water wasn't mentioned before that. So yeah, if anyone knows what to do it would be much appreciated.
Edit: replaced "a" with "some".
A series of measurements are made in order to determine the molar mass of an unknown gas. First, a flask is evacuated and found to weigh 134.567 g. It is then filled with the gas to a pressure of 735 mm Hg at 31 degrees C and found to weigh 1067.9 g. (The density of the water at this temperature is 0.997 g/ml.) Assuming that the ideal-gas equation applies, calculate the molar mass of the unknown gas.
Yeah, I've looked at this for a while and can't really see what to do, I swear it doesn't give enough information. And then it says "the" water, a definite article instead of using "some" (or not using an article at all) the indefinite article, but water wasn't mentioned before that. So yeah, if anyone knows what to do it would be much appreciated.
Edit: replaced "a" with "some".