Question

At constant pressure, a 1.10 l container decreases in volume to 222 ml. what is the final temperature if the initial temperature is 31.0 ℃?

a) 61.4℃
b) 61.4 k
c) 6.26 ℃
d) 6.26 k

Answer 1

The final temperature of the gas is 61.4 K. Hence, the correct answer to this question is option b).

Step-by-step explanation:

The student's question involves applying Charles's Law, which is a gas law stating that at constant pressure, the volume of a given mass of an ideal gas is directly proportional to its absolute temperature. To find the final temperature of the gas, we can use the combined gas law equation, which states that:

P₁V₁/T₁ = P₂V₂/T₂. Given that the initial volume (V₁) is 1.10 L, the final volume (V₂) is 222 mL (or 0.222 L), the initial temperature (T₁) is 31.0 ℃ (or 304.15 K), and the pressure (P) remains constant, we can rearrange the equation to solve for the final temperature (T₂). Plugging in the values, we get:

P₁V₁/T₁ = P₂V₂/T₂. 1 atm * 1.10 L / 304.15 K = 1 atm * 0.222 L / T₂. From here, we can solve for T₂:. T₂ = (1 atm * 0.222 L * 304.15 K) / (1 atm * 1.10 L). T₂ = 61.4 K. Therefore, the final temperature is 61.4 K.