Question

calculate the final pressure of a gas that is expanded from 725cm³ at 30C and 1.19 atm to 1.12cm³ at 43C​

Answer 1

Final pressure, P2 = 1088.89 atm

Step-by-step explanation:

Given the following data;

• Initial volume, V1 = 725 cm³
• Initial temperature, T1 = 30°C
• Initial pressure, P1 = 1.19 atm
• Final volume, V2 = 1.12 cm³
• Final temperature, T2 = 43°C

To find the final pressure (P2), we would use the combined gas law.

Mathematically, the combined gas law is given by the formula;

`\frac {PV}{T} = k`

`\frac {P_(1)V_(1)}{T_(1)} = \frac {P_(2)V_(2)}{T_(2)}`

Substituting into the formula, we have;

`\frac {1.19*715}{30} = \frac {P_(2)*1.12}{43}`

`\frac {850.85}{30} = \frac {P_(2)*1.12}{43}`

`28.3617 = \frac {P_(2)*1.12}{43}`

Cross-multiplying, we have;

`28.3617 * 43 = 1.12P_(2)`

`1219.5531 = 1.12P_(2)`

`P_(2) = \frac {1219.5531}{1.12}`

Final pressure, P2 = 1088.89 atm