The Ideal Gas Law is given by the equation: PV=nRT PV = nRT PV=nRT where:
From the problem, we have:
The ideal gas constant R R R is 0.0821 0.0821 0.0821 L·atm/(mol·K).
Rearrange the equation to solve for V V V: V=nRTP V = \frac{nRT}{P} V=PnRT
Substitute the values into the equation: V=(0.627 mol)(0.0821 L\cdotpatm/(mol\cdotpK))(287 K)1.06 atm V = \frac{(0.627 \, \text{mol}) (0.0821 \, \text{L·atm/(mol·K)}) (287 \, \text{K})}{1.06 \, \text{atm}} V=1.06atm(0.627mol)(0.0821L\cdotpatm/(mol\cdotpK))(287K)
Perform the calculation: V=(0.627)(0.0821)(287)1.06 V = \frac{(0.627) (0.0821) (287)}{1.06} V=1.06(0.627)(0.0821)(287) V=14.73571.06 V = \frac{14.7357}{1.06} V=1.0614.7357 V≈13.9007 L V \approx 13.9007 \, \text{L} V≈13.9007L
The volume occupied by 0.627 mol of nitrogen gas at a pressure of 1.06 atm and a temperature of 287 K is: 13.9007 L \boxed{13.9007 \, \text{L}} 13.9007L
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