Question

1.09 g of h2 is contained in a 2.00 l container at 20.0 °c. What is the pressure in this container in mmhg? 49.3012 493.012 mm hg 4930.12 mm hg 49301.2

Answer 1

Answer: The pressure in this container in 4940 mmHg so the nearest option is 4930.12 mmHg.

Explanation:

According to ideal gas equation:

PV=nRT

Given :

Volume of the container = 2 liters

P = pressure of the gas in in container = ?atm

R = Universal gas constant = $0.082 L atm K^{-1} mol^{-1}$

T= temperature in kelvins = $20^oC=20+273.15 K= 293.15 K(0^oC=273.15 K)$

n=number of moles =$\frac{\text{mass of the gas}}{\text{molecular mass of the gas}}=\frac{1.09 g}{2 g/mol}=0.545 mol$

Substituting values in ideal gas equation :

$(2.00 L)(P)=(0.545 mol)(0.082 L atm K^{-1} mol^{-1})(293.15 K)$

$P=6.5 atm=6.5\times 760 mmHg=4940 mmHg$  (1 atm=760 mmHg)

The pressure in this container in 4940 mmHg.