An engineer pumps 5.00 mol of carbon monoxide gas into a cylinder that has a capacity of 20.0L. What is the pressure In kPa of gas inside the cylinder at 25 °C?

*use the ideal gas law*

The pressure of the cylinder is 619.1 kPa

Explanation:

To calculate the pressure, we use the equation given by ideal gas which follows:

where,

P = pressure of the gas = ?

V = Volume of the gas = 20.0 L

T = Temperature of the gas =

R = Gas constant =

n = number of moles of CO gas = 5.00 moles

Putting values in above equation, we get:

Hence, the pressure of the cylinder is 619.1 kPa

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.