What will be the pressure exerted by 16 g of methane in a 250 mL container at 300 K using ideal gas equation?

Question

What will be the pressure exerted by 16 g of methane in a 250 mL container at 300 K using ideal gas equation? (A) 9.852 atm (B) 98.52 atm (C) 985.2 atm (D) None of these

Tardigrade Admin · Accepted Answer

Given, 16 g of CH 4=(16/16)=1 mol The ideal gas equation predicts that the pressure exerted will be, P=(n R T/V)=(1 × 0.0821 × 300/0.250)=98.52 atm

Q. What will be the pressure exerted by $16 g$ of methane in a $250 m L$ container at $300 K$ using ideal gas equation?

$9.852 a t m$

$98.52 a t m$

$985.2 a t m$

None of these

Given, $16 g$ of $C H_{4} = \frac{16}{16} = 1 m o l$

The ideal gas equation predicts that the pressure exerted will be,

$P = \frac{n RT}{V} = \frac{1 \times 0.0821 \times 300}{0.250} = 98.52 a t m$

Q. What will be the pressure exerted by 16g of methane in a 250mL container at 300K using ideal gas equation?

9.852atm

98.52atm

985.2atm