Question

At 20 Celsus the volume of hydrogen occupies 12.05L at 100.1kPa. What is the new volume if the pressure increases to 120.0kPa and the temperature remain constant

Answer 1

Answer:

0.0987

EXPLANATION:

from boyles law, which state that the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature. i.e

= $V₂P₂=$P₁V₁

$V₂=P₁V₁/P₂$

FROM THE GIVEN PARAMETERS

P₁ (initial pressure)=1001.1kpa

P₂(final pressure)=120.0kpa

but 1kpa = 0.0987atm, converting to atm

P₂(final pressure)=1.184 atm

T=constant

V₁=12.05L

FROM THE BOYLE'S LAW FORMULAR

$V₂P₂=$P₁V₁

$V₂=P₁V₁/P₂$

=

V₂=0.987×12.05/1.184

=10.04L

V₂ = 10.04L

Answer 2

Answer:

10.04L

Explanation:

According to Boyle's law, volume is inversely proportional to pressure when the temperature is constant or in other words under a constant temperature when the pressure on a gas increases its volume decreases.

Formula:

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

Given:

Initial pressure $P_{1}$= 100.1kPa => 0.987 atm

Initial volume $V_{1}$= 12.05L

Final pressure $P_{2}$= 120.0kPa=> 1.184 atm

Temperature is constant

Required:

Final volume $V_{2}$=? L

Solution:

Re arranging the formula,

$V_{2}$= ( $P_{1}$x$V_{1}$ )/$P_{2}$

$V_{2}$= (0.987x12.05)/ 1.184

$V_{2}$=  10.04L

the new volume is 10.04 L