Using the ideal gas law equation:
P1V1 / n1T1 = P2V2 / n2T2
Since pressure and temperature are constant, the equation simplifies to:
V1 / n1 = V2 / n2
Plugging in the numbers given:
23.5 L / 15.0 mol = 1.70 L / x
x = (1.70 L * 15.0 mol) / 23.5 L
x = 1.08 mol
Therefore, the sample of oxygen gas in the 1.70 L volume contains 1.08 mol of oxygen gas.
A sample of oxygen gas contains 15.0 mol in a volume of 23.5 L. If the pressure and temperature are kept constant, but the volume is changed to 1.70L , how many moles of oxygen gas does the sample contain? Be sure your answer has the correct number of significant figures.
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