To solve this problem, we can use the combined gas law equation:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = 270 mmHg
V1 = 400 ml
T1 = 65C + 273 = 338K
P2 = 1.4 atm
V2 = unknown
T2 = 100C + 273 = 373K
Now we can plug in the values and solve for V2:
(270 mmHg * 400 ml) / (338K) = (1.4 atm * V2) / (373K)
(108000) / (338) = 1.4V2 / 373
318.93 = 1.4V2 / 373
1.4V2 = 118.58
V2 = 118.58 / 1.4
V2 ≈ 84.7 ml
Therefore, the new volume of the gas at 1.4 atm and 100C is approximately 84.7 ml.
An ideal gas occupies 400ml at 270 mmHg and 65C. If the pressure is changed to 1.4 atm and the temperature is increased to 100C, what is the new volume?
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