A sample of 0.0200 mol of chlorine gas is kept at 27.0°c and 0.150 atm. what would be its pressure if the temperature was increased to 227.°c and the volume kept the same

Question

Travis Barron

Chemistry

9 September, 09:31

A sample of 0.0200 mol of chlorine gas is kept at 27.0°c and 0.150 atm. what would be its pressure if the temperature was increased to 227.°c and the volume kept the same

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Bubbles · Answer 1

Answer is: 0,250 atm.

T₁ (chlorine) = 27°C = 300K.

T₂ (chlorine) = 227°C = 500K.

T₂/T₁ = 1,66.

p1 (chlorine) = 0,150 atm.

p2 (chlorine) = ?

V (chlorine) = constant.

n (chlorine) = 0,0200 mol.

R - gas constant, R = 0.0821 atm·l/mol·K.

Ideal gas law: p·V = n·R·T.

p = n·R·T:V.

If temperature was increased 1,66 times, pressure also increase 1,66 times: 1,66·0,150 atm = 0,250 atm.