The temperature of 2.0 g of helium is increased at constant volume by ΔT. What mass of oxygen can have its temperature increased by the same amount at constant volume using the same amount of heat?
I know for constant volume I should use the equation: Q=mCsubvdeltaT
I also know that in my book Molar specific heats of gases (J/mol*K) at 20degrees Celcius:
Csubv of Helium = 12.5
Csubv of Oxygen = 20.9
How do I set up this equation and solve it?
To solve this problem, we will use the principles of heat transfer and the equation you mentioned: Q = m * Csubv * ΔT.
First, let's calculate the heat transferred to the helium using the equation Q = m * Csubv of helium * ΔT:
Qhelium = (2.0 g) * (12.5 J/mol*K) * ΔT.
Next, we need to find the mass of oxygen that can have the same temperature increase at constant volume. Since the heat transfer is the same for both gases, we can set up the equation Qhelium = Qoxygen:
(2.0 g) * (12.5 J/mol*K) * ΔT = moxygen * (20.9 J/mol*K) * ΔT.
Now, we can solve for the mass of oxygen (moxygen):
moxygen = (2.0 g) * (12.5 J/mol*K) / (20.9 J/mol*K).
Simplifying the expression gives us:
moxygen = 1.198 g.
Therefore, 1.198 grams of oxygen can have its temperature increased by the same amount at constant volume using the same amount of heat.