Question

4. Fifty liters of hydrogen gas is at a temperature of -10 C and 780 torr pressure. What would be the volume of this gas at standard temperature and pressure 5. What temperature in degrees Celsius is required to change 200 ml of nitrogen gas at 25 C to a volume of 250 ml? This problem is an example of which gas law?

Answer 1

. For ideal gas we know, PV = nRT P= 280 tory = 780 atm = 1.026 alom T= -10°C = (273-10) K = 263k Here V- SOL to R20.082 L-ahm mapa K 1.026 atm x 50 h = nx 0.082 L-aho max 263k Now or; n = 2.38 moles. the standard temperature and pressure Pa sahm, tzoc 2273k is: 1 atm x v = 2.38 mol x 0.082 L-atmamak x 273K N = 53.28 L So the volume of the gas is 58.28 L Again we know for ideal gas 1 mole of gas at std. T and P occupy 22.0L of volname. Here the the gas present = 2.38 moles So the volume occupy = 2214 x2:38 L 2 53.31L This value is so close (53.28L) to the Calenlated value.

pressure Iso For ideal gas we know, Na T at constant temp and mole number This is charles gas Law . 200 ml 98k Given that wi= 200 ml , It = 25°c = (273 +25)k = 298k 2 = 250 ml, T2 =?. So 200 ml = 298k or, T = 372.5k T2 = (37215 - 2730% = 9915.c Temp. is required. This problem is an example of Charles gas law.