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10.0 grams of a gas occupies 12.5 liters at a pressure of 42.0 mm Hg What is the volume when the pressure has increased to 75.0 mm Hg?
Wiki User
∙ 11y ago
Using Boyle's Law, p1*V1= p2*V2. This means that the pressure multiplied by the volume remains constant whilst the temperature is the same.
Therefore; p1=42.0mm Hg, V1= 12.5L and so the product of the two is 525.
If the pressure is now 75 mm Hg the volume must be 525/75= 7 liters.
The 10.0 grams of gas information is not needed.
Wiki User
∙ 11y ago
Wiki User
∙ 12y agoat STP convert 0degrees C to Kelvin = 273K
then convert 35degrees C to Kelvin = 308K
use equation (V1/T1)=(V2/T2)
V1 = 22.4L
T1 = 273K
V2 = ?
T2 = 308K
plug in numbers and this is your answer.
Wiki User
∙ 11y agoThe molar volume of any gas at a pressure of 1 bar and a temperature of 20 0C is after CODATA (2010) 24,789 598(42).
Wiki User
∙ 7y agoThe temperature is 260 K.
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