Question

At a temperature of __________ °c, 0.444 mol of co gas occupies 11.8 l at 889 torr.

Answer 1

ideal gas law is: PV = nRT P = pressure (torr) = 889 torr V = volume (Liters) = 11.8 L n = moles of gas = 0.444 mol R = gas constant = 62.4 (L * torr / mol * k) solve for T (in kelvin) T = PV/nR T = (889*11.8)/(.444*62.4) T = 378.6 K convert to C (subtract 273) T = 105.6 deg C

Answer 2

Answer:
`106^0C`

Explanation: IDEAL GAS LAW

`PV=nRT`

where,

P = pressure of the gas = 889 torr = 1.17 atm (1 torr=0.0013atm)

V = volume of the gas = 11.8 L

T = temperature of the gas = ? K

n = number of moles of gas = 0.444

R = Gas constant = 0.0821 Latm/moleK

`1.17* 11.8=0.444* 0.0821* T`

`T=379K`

`T=(379-273)^0C=106^0C`

Thus temperature of gas is
`106^0C`