Question

1. Calculate the volume of the gas, in liters, if 1.55 mol has a pressure of 1.20 atm at a temperature of -6 ∘C. (Answer in L)

2.Calculate the absolute temperature of the gas at which 3.33×10⁻³ mol occupies 498 mL at 760 torr . (Answer in K)

3.Calculate the pressure, in atmospheres, if 2.65×10⁻³ mol occupies 415 mL at 140 ∘C. (Answer in atm)

4.Calculate the quantity of gas, in moles, if 127 L at 60.0 ∘C has a pressure of 11.15 kPa .(Answer in moles)

Thanks!

Answer 1

(1) To find the volume of the gas Use the ideal gas law: PV = nRT p= pressure n=n moles of any gas R = gas constant T = temperature in kelvin v= volume p= 120 atm n = 1.55 mol R = 0.0821L atm/mol. K T=-6+273K = 267K V=? P v-155molx0.0821L - atm /mol Kx267K 1.20 atm = 28.3L Hence the volume of the gas = 28.3L

To find the temperature of the gas Use the ideal gas law : PV = nRT T-PV nR p = 760 torr latm = 760 torr n = 333x 10-mol R = 0.0821L atm/mol.K T = ? V =498 mL = 0.498L T - DV InR latm x0.498L T= 3.33x10 mol 0.0821L-atm/mol. K = 1821K Hence the temperature of the gas = 1821K

(3) To find the pressure of the gas Use the ideal gas law: p = ? n = 2.65 x 10-mol R = 0.0821Latm/mol. K T = 140+273 = 413K V =415mL = 0.415L P=nRT V 2.65x10 mol x 0.0821L.atm/mol Kx413K 0.415L = 0.216 atm Hence the pressure of the gas = 0.216 atm (4) To find the moles of the gas Use the ideal gas law : PV = nRT p= 11.15 kPa Convert pressure kPa to atm latm = 101.325kPa 1kPa=- 101 325 atm 1 11.15 kPa = 1115x a tm = 0.110atm P=0.110atm n = ? R = 0.0821 L atm /mol-K T = 60.0+273K = 333K V=127 L PV = RT 0.110atm 127 L 0.0821L atm/mol.Kx333K = 0.510 moles Hence the moles of the gas = 0.510 moles