0.5 moles of gas A and x moles of gas B exert a pressure of 200 Pa in a container of volume 10 m³ at 1000 K. Given R is the gas constant in JK⁻¹ mol⁻¹, x is
(A) 2R/(4 + R)
(B) 2R/(4 - R)
(C) (4 + R)/2R
(D) (4 - R)/2R
[JEE Main 2019]
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Answer:
4+R / 2R is answer is the option c
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the value of x is (D) (4 - R)/2R
- Pressure of B, P₂ = mole fraction of B × total pressure
P₂ = {x/(x + 0.5)}×P
- From the ideal gas equation ,
P₂ × V = n × R × T
P₂ = x × R × T / V ( n = x = no. of moles )
- From the above equations,
{x/(x + 0.5)} × P = x × R × T/V
Putting the values,
(x/x + 0.5) × 200 = x × 8.314 × 1000/10
On solving this,
We get,
x = (4 - R/2R)
- so the correct answer is option (D)
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