the volume of a sample of gas is 750ml at 75 degree celsius and 0.750atm.at what temperature in celsius will the sample occupy 1.000L under a pressure of 1.000atm?
(P1V1/T1) = (P2V2/T2)
Don't forget T must be in kelvin.
Ahahha
The volume of a sample of a gas is 750 ml at 60 degrees celsius and 0.7 atm. At what temperature will the sample of 1.00 L occupy under a pressure of 1.00 atm?
To solve this problem, we will use the combined gas law equation:
(P₁V₁) / T₁ = (P₂V₂) / T₂
Where:
P₁ and P₂ are the initial and final pressures,
V₁ and V₂ are the initial and final volumes, and
T₁ and T₂ are the initial and final temperatures
Let's fill in the given values first:
P₁ = 0.750 atm
V₁ = 750 mL = 0.750 L
T₁ = 75 °C
P₂ = 1.000 atm
V₂ = 1.000 L
T₂ = X (The value we need to find)
Now, we can plug in the values into the combined gas law equation and solve for T₂:
(0.750 atm * 0.750 L) / (75 °C) = (1.000 atm * 1.000 L) / (T₂)
Rearranging the equation to solve for T₂, we have:
T₂ = (1.000 atm * 1.000 L * 75 °C) / (0.750 atm * 0.750 L)
T₂ = 100 °C
Therefore, the sample of gas will occupy 1.000 L under a pressure of 1.000 atm at a temperature of 100 °C.