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Question
Solve the following.
At 25°C and 760 mm of Hg pressure, a gas occupies 600 mL volume. What will be its pressure at the height where the temperature is 10°C and the volume of the gas 640 mL?
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Solution
Given:
V1 = Initial volume = 600 mL,
V2 = Final volume = 640 mL
P1 = Initial pressure = 760 mm Hg
T1 = Initial temperature = 25°C = 25 + 273.15 K = 298.15 K
T2 = Final temperature = 10°C = 10 + 273.15 K = 283.15 K
To find: P2 = Final pressure
Formula: `("P"_1"V"_1)/"T"_1=("P"_2"V"_2)/"T"_2`
Calculation:
According to combined gas law,
`("P"_1"V"_1)/"T"_1=("P"_2"V"_2)/"T"_2`
∴ `P_2 = ("P"_1"V"_1"T"_2)/("T"_1"V"_2)`
∴ `P_2 =(760xx600xx283.15)/(298.15xx640)`
∴ P2 = 676.654 mm Hg
The final pressure of a gas is 676.654 mm Hg.
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