2. A quantity of 1.12 moles of gas at 25 ºC exhibits a pressure of 980 torr and occupies a volume of 4.12 L. a?
2. A quantity of 1.12 moles of gas at 25 ºC exhibits a pressure of 980 torr and occupies a volume of 4.12 L. a) Calculate the pressure of the gas if 1.00 moles of the same gas are added at constant volume and temperature. b) Calculate the new temperature of the gas after adding 1.00 moles of gas at constant pressure and volume
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p1V1 / p2V2 = n1 T1 / n2 T2
980 /760 = 1.29 atm
25 + 273 = 298 K
1.29 atm x 4.12 / p2 x 4.12 = 1.12 x 298 K / 2.12 x 298
basically
1.29 / p2 = 1.12 / 2.12
p2 = 2.44 atm
p1V1 = p2V2
p1V1 / p2V2 = 1
1 = 1.12 x 298 / 2.12 T2
2.12 T2 = 1.12 x 298
T2 = 157 K => - 115 °C