# Given that 6.6 moles of carbon monoxide gas are present in a 43.3L container, what is the pressure of the gas (in atm) if the temperature is 84°C?

##### 1 Answer

#### Answer:

#### Explanation:

This is a straightforward application of the ideal gas law equation.

#color(blue)(PV = nRT)" "# , where

Notice that the question provides you with

the number of moles of gasthe volume of the containerthe temperature of the gas

This means that you have everything you need to calculate the pressure of the gas, provided that you know the value of the *universal gas constant*

#R = 0.082("atm" * "L")/("mol" * "K")#

Plug in your values into the above equation and solve for

#PV = nRT implies P = (nRT)/V#

#P = (6.6color(red)(cancel(color(black)("moles"))) * 0.082("atm" * color(red)(cancel(color(black)("L"))))/(color(red)(cancel(color(black)("mol"))) * color(red)(cancel(color(black)("K")))) * (273.15 + 84)color(red)(cancel(color(black)("K"))))/(43.3color(red)(cancel(color(black)("L"))))#

#P = "4.464 atm"#

Round this off to two sig figs, the number of sig figs you gave for the number of moles of gas

P = color(green)("4.5 atm")#