Chapter 11.4, Problem 11.41QAP

Interpretation Introduction

Interpretation:

The final pressure of isoflurane in atmosphere should be calculated when the gas is warmed to a temperature of 22°C, under conditions of constant volume and amount of gas. Given that the gas is at initial pressure of 1.8 atm and temperature of 5°C.

Concept introduction:

► The relation between pressure (P) and temperature (T) of a gas under constant volume and amount of the gas is represented through Gay-Lussac’s Law.

► As per Gay-Lussac’s law, pressure is directly related to temperature:

$\begin{array}{l}\text{P α T i}\text{.e}\text{. P = k}\times \text{T}\\ \text{where 'k' is the proportionality constant}\\ (\text{or})\frac{{\text{P}}_{\text{1}}}{{\text{T}}_{\text{1}}}\text{ = }\frac{{\text{P}}_{\text{2}}}{{\text{T}}_{\text{2}}}-----(1)\\ {\text{where P}}_{\text{1}}{\text{ and P}}_{\text{2}}\text{ are the initial and final pressures}\\ {\text{T}}_{\text{1}}{\text{ and T}}_{\text{2}}\text{ are the initial and final temperature}\end{array}$

► The standard units for pressure is atmosphere (atm) and temperature kelvin (K)

► Pressure conversions:

1 torr = 1 mmHg

1 atm = 760 torr = 760 mmHg

Temperature conversion:

K =°C + 273 (or) °C = K - 273

Given:

Initial pressure P₁ = 1.8 atm

Initial temperature T₁ = 5°C = (5 + 273) K = 278 K

Final temperature T₂ = 22°C = (22 + 273) K = 295 K

Final pressure = P₂