QuestionJuly 14, 2025

What is the final temperature of a system with a volume of 88.70mL with an initial temperature of 56.00 Celsius and the volume increases to 899.0mL? 242.4K 32.46K 3335K 57.98K

What is the final temperature of a system with a volume of 88.70mL with an initial temperature of 56.00 Celsius and the volume increases to 899.0mL? 242.4K 32.46K 3335K 57.98K
What is the final temperature of a system with a volume of 88.70mL with an initial temperature of 56.00 Celsius and the volume increases to 899.0mL? 242.4K 32.46K 3335K 57.98K

Solution
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Answer

3335K Explanation 1. Identify the Law Use Charles's Law for gases, which states that \frac{V_1}{T_1} = \frac{V_2}{T_2}, where V is volume and T is temperature in Kelvin. 2. Convert Initial Temperature to Kelvin T_1 = 56.00 + 273.15 = 329.15 \text{ K} 3. Apply Charles's Law Rearrange to find T_2: T_2 = T_1 \times \frac{V_2}{V_1} 4. Calculate Final Temperature T_2 = 329.15 \times \frac{899.0}{88.70} = 3335 \text{ K}

Explanation

1. Identify the Law<br /> Use Charles's Law for gases, which states that $\frac{V_1}{T_1} = \frac{V_2}{T_2}$, where $V$ is volume and $T$ is temperature in Kelvin.<br /><br />2. Convert Initial Temperature to Kelvin<br /> $T_1 = 56.00 + 273.15 = 329.15 \text{ K}$<br /><br />3. Apply Charles's Law<br /> Rearrange to find $T_2$: $T_2 = T_1 \times \frac{V_2}{V_1}$<br /><br />4. Calculate Final Temperature<br /> $T_2 = 329.15 \times \frac{899.0}{88.70} = 3335 \text{ K}$
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