You transfer a sample of a gas at 17°C from a volume of 5.67 L and 1.10 atm to a container at 37°C that has a pressure of 1.10 atm. The new volume of the gas will be 6.06 L.
This law combined the three gas laws that is (i) Charle's Law (ii) Gay-Lussac's Law and (iii) Boyle's Law
It is expressed as
[tex]\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}[/tex]
where
P₁ = first pressure
P₂ = second pressure
V₁ = first volume
V₂ = second volume
T₁ = first temperature
T₂ = second temperature
Convert temperature Celsius into Kelvin
T(K) = T(°C) + 273
T₁(K) = 17 + 273
= 290 K
T₂(K) = 37 + 273
= 310 K
Now put the value in above formula we get
[tex]\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}[/tex]
[tex]\frac{1.10 \times 5.67}{290} = \frac{1.10 \times V_2}{310}[/tex]
[tex]V_{2} = \frac{1.10 \times 5.67 \times 310}{290 \times 1.10}[/tex]
V₂ = 6.06 L
Thus from the above conclusion we can say that The new volume of the gas will be 6.06 L.
Learn more about the Combined gas Law here: https://brainly.com/question/25587265
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