Question

1. Determine the pressure change when a constant volume of gas at3.00 atm is heated from 25.0 °C to 36.0 °C.

Answer 1

The pressure change = 3.11 atm

Step-by-step explanation

Given:

Initial pressure, P₁ = 3.00 atm

Initial temperature, T₁ = 25.0 °C = (25.0 + 273.15 K) = 298.15 K

Final temperature, T₂ = 36.0 °C = (36.0 + 273.15 K) = 309.15 K

What to find:

The final pressure, P₂.

Step-by-step solution:

The final pressure, P₂ of the gas can be calculated using the Amonton's law equation/formula given below:

`\begin{gathered} (P_1)/(T_1)=(P_2)/(T_2) \\ \\ \Rightarrow P_2=(P_1T_2)/(T_1) \end{gathered}`

Putting the values of the parameters into the formula, we have:

`P_2=\frac{3.00\text{ }atm*309.15\text{ }K}{298.15\text{ }K}=3.11\text{ }atm`

Therefore, the pressure change when a constant volume of gas at

3.00 atm is heated from 25.0 °C to 36.0 °C = 3.11 atm.