Question

A gas occupies a volume of 2.67 Times 10 to the square root of two mL at 542.48 mm Hg pressure. What will be its volume at constant temperature if the pressure is changed to 778.05MM Hg

Answer 1

Answer:

The volume of the gas at constant temperature is:

186.16 mL

Explanation:

Byole's Law : The pressure exerted by the fixed amount of gas is inversely proportional to Volume at the constant temperature.

$P=k\frac{1}{V}$

Here k = proportionality constant

$PV= k$

If P1 and V1 are initial pressure and Volume of gas and P2 , V2 are final volume of the gas , Then :

$P_{1}V_{1}=P_{2}V_{2}$

P1 = 542.48 mm Hg

$V_{1} =2.67\times 10^{2}mL$

P2 = 778.05 mm Hg

Insert the values of P1 , V1 and P2 in formula and calculate V2

$P_{1}V_{1}=P_{2}V_{2}$

$542.48\times 2.67\times 10^{2}=778.05V_{2}$

dividing the equation by 778.05

$V_{2}=\frac{542.48\times 2.67\times 10^{2}}{778.05}$

$542.48\times 2.67\times 10^{2}mL= 144842.16$

$V_{2}=\frac{144842.16}{778.05}$

$V_{2}=186.16mL$