Question

A sample of ammonia gas at 298 K has a volume of 3.5 L at a pressure of 170.2 kPa, what is the new pressure if the gas is compressed to a volume of 1.35 L at 293 K?

Answer 1

The final pressure of the gas comes out to be 433.85 KPa

Step-by-step explanation:

Initial volume of gas = V = 3.5 L

Initial pressure of gas = P = 170.2 KPa

Initial temperature = T = 298 K

Final volume of gas = V' = 1.35 L

Final temperature of gas = T' = 293 K

Assuming the number of moles of gas remains constant.

The final pressure of the gas is obtained by the following equation shown below

`\displaystyle (PV)/(T) = \displaystyle (P'V')/(T') \\\displaystyle \frac{170.2 \textrm{ KPa}* 3.5 \textrm{ L}}{298\textrm{ K}} = \displaystyle \frac{P'* 1.35 \textrm{ L}}{293 \textrm{ K}} \\P' = 433.85 \textrm{ KPa}`

Final pressure of gas = 433.85 KPa

Answer 2

430 kPa

Step-by-step explanation:

Use the formula PV/T = PV/T where the left side of the equation refers to the initial values and the right side refers to the final values: (170.2 kPa)(3.5 L)/(298 K) = (P)(1.35 L)/(293 K). The P represents the unknown pressure. Solving this equation gives us a value for P of 433.855 kPa, but because of significant figures (the two from 3.5 L), we round to 430 kPa.