Question

A sample of N2 gas in a flask is heated from 27 Celcius to 150 Celcius. If the original gas is @ pressure of 1520 torr, what is the pressure of the final sample (in atm)?A.) 1.4atmB.) 2.8atmC.) 3.2atmD.) 4.3atm

Answer 1

`\large \boxed{\text{B.) 2.8 atm}}`

Step-by-step explanation:

The volume and amount are constant, so we can use Gay-Lussac’s Law:

At constant volume, the pressure exerted by a gas is directly proportional to its temperature.

`(p_(1))/(T_(1)) = (p_(2))/(T_(2))`

Data:

p₁ = 1520 Torr; T₁ = 27 °C

p₂ = ?; T₂ = 150 °C

Calculations:

(a) Convert the temperatures to kelvins

T₁ = ( 27 + 273.15) K = 300.15 K

T₂ = (150 + 273.15) K = 423.15 K

(b) Calculate the new pressure

`\begin{array}{rcl}(1520)/(300.15) & = & (p_(2))/(423.15)\\\\5.064 & = & (p_(2))/(423.15)\\\\5.064*423.15&=&p_(2)\\p_(2) & = & \text{2143 Torr}\end{array}\\`

(c) Convert the pressure to atmospheres

`p = \text{2143 Torr} * \frac{\text{1 atm}}{\text{760 Torr}} = \textbf{2.8 atm}\\\\\text{The new pressure reading will be $\large \boxed{\textbf{2.8 atm}}$}`