The volume of a gas is 200 mL at 315.0 kPa pressure. What will the volume be
when the pressure is reduced to 50.0 kPa, assuming the temperature remains
constant?

1260 mL

Explanation:

Given data:

Initial volume of gas = 200 mL

Initial pressure = 315.0 KPa

Final volume = ?

Final pressure = 50.0 KPa

Solution:

"The volume of given amount of gas is inversely proportional to its pressure by keeping the temperature and number of moles constant"

Mathematical expression:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = initial volume

P₂ = final pressure

V₂ = final volume  

Now we will put the values in formula,

P₁V₁ = P₂V₂

315 KPa × 200 mL = 50 KPa × V₂

V₂ = 63000 KPa. mL/ 50 KPa

V₂ = 1260 mL

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.