?Calculate each of the following quantities for an ideal gas: (a) the volume of the gas, in liters, if 1.50 mol has a pressure of 1.25 atm at

Chapter 10, Problem 10.34

(choose chapter or problem)

Calculate each of the following quantities for an ideal gas:

(a) the volume of the gas, in liters, if 1.50 mol has a pressure of 1.25 atm at a temperature of \(-6^{\circ} \mathrm{C}\);

(b) the absolute temperature of the gas at which \(3.33 \times 10^{-3} \mathrm{~mol}\) occupies 478 mL at 750 torr;

(c) the pressure, in atmospheres, if 0.00245 mol occupies 413 mL at \(138^{\circ} \mathrm{C}\);

(d) the quantity of gas, in moles, if 126.5 L at \(54^{\circ} \mathrm{C}\) has a pressure of 11.25 kPa.

Text Transcription:

-6^{\circ} C

3.33 \times 10^{-3} mol

138^{\circ} C

54^{\circ} C