A sample of gas contains 0.1200 mol of OF2(g) and 0.1200 mol of H2O(g) and occupies a volume of 7.92 L. The following reaction takes place:
Before we have n1=0,12+0,12=0,24 mol of gas, After the reaction takes place we have n2=0,12+2*0,12=0,36 mol of gas. Let's call V1 the volume before and V2 the volume after
PV1=n1RT (Ideal Gas Law)
so V2=V1*N2/N1=11,88 L
Correct!! can u do this one for me i don't have time to post!
Compute the root-mean-square speed of H2 molecules in a sample of hydrogengas at a temperature of 74°C.
that one wasn't right
What value do you have ?
i put 65.8
the error is from the fact that I have put 2 for M
I should put M=0,002 kg/mol (SI units)
so the right answer is 2080 m/s
At the first sight, the first answer seems too low for me. This one is more realistic.
Right! one more please ! im in a hurry
Compute the root-mean-square speed of Ar molecules in a sample of argon gas at a temperature of 174°C.
1.32 mol sample of oxygen gas at a temperature of 9.00 °C is found to occupy a volume of 28.1 liters. The pressure of this gas sample is mm Hg.
A sample of nitrogen gas collected at a pressure of 663 mm Hg and a temperature of 279 K has a mass of 15.5 grams. The volume of the sample is L.
826 mmHg and
The average molecular speed in a sample of Kr gas is 306 m/s at 370 K. The average molecular speed in a sample of Ar gas is m/s at the same temperature.
The rate of effusion of Kr gas through a porous barrier is observed to be 2.30E-4 mol / h. Under the same conditions, the rate of effusion of Xe gas would be mol / h.
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