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Question
Solve the following.
At 0°C, a gas occupies 22.4 liters. How much hot must be the gas in celsius and in kelvin to reach a volume of 25.0 liters?
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Solution
Given:
V1 = Initial volume of the gas = 22.4 L,
T1 = Initial temperature = 0 + 273.15 = 273.15 K,
V2 = Final volume = 25.0 L
To find: T2 = Final temperature in Celsius and in Kelvin
Formula: `"V"_1/"T"_1="V"_2/"T"_2` (at constant n and P)
Calculation:
According to Charles’ law,
`"V"_1/"T"_1="V"_2/"T"_2` (at constant n and P)
∴ T2 = `("V"_2xx"T"_1)/"V"_1`
∴ T2 = `(25.0xx273.15)/22.4` = 304.85 K ≈ 304.9 K
Converting to Celsius scale:
304.85 K = 304.85 − 273.15°C = 31.7°C
The temperature of the gas must be 31.7°C or 304.9 K
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