A sample of sulfur hexafluoride gas (SF6) occupies a volume of 3.230 Liters at 7.011 x 101 oC. Assuming the pressure is constant, what will the final temperature be (in o C) if the volume is increased to 7.350 Liters?
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Use (v1/t1) = (v2/t2)
Remember to change the T to kelvin.
To determine the final temperature, we can use the combined gas law equation, which relates the initial and final states of a gas sample when pressure and amount of gas are constant.
The combined gas law equation is as follows:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 and P2 are the initial and final pressures, which are assumed to be constant.
V1 and V2 are the initial and final volumes.
T1 and T2 are the initial and final temperatures.
Based on the given information, we can write the equation as:
(P * 3.230 L) / (7.011 x 10^1 oC) = (P * 7.350 L) / T2
Since the pressure (P) is considered constant, we can simplify the equation to:
(3.230 L) / (7.011 x 10^1 oC) = (7.350 L) / T2
Now we can solve for T2 by rearranging the equation as follows:
T2 = (7.350 L * 7.011 x 10^1 oC) / (3.230 L)
T2 ≈ 15.894 x 10^1 oC
Therefore, the final temperature, when the volume is increased to 7.350 Liters, will be approximately 158.94 °C.