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

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

= P₁V₁

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

P₁V₁

=

V₂=0.987×12.05/1.184

=10.04L

V₂ = 10.04L

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:

/ = /

Given:

Initial pressure = 100.1kPa => 0.987 atm

Initial volume = 12.05L

Final pressure = 120.0kPa=> 1.184 atm

Temperature is constant

Required:

Final volume =? L

Solution:

Re arranging the formula,

= ( x )/

= (0.987x12.05)/ 1.184

=  10.04L

the new volume is 10.04 L

1.195000

explanation:

total mass=0.0117+0.0137+0.0881+0.0111

total mass= 0.01172kg

total velocity = 0.283-0.743+0.871-0.799+0.155+0.637+0.301=0.102

momentum=mv=0.1172*0.102=1.195000//