To solve this problem, we can use the combined gas law equation:
(P1/T1) = (P2/T2)
where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.
Plugging in the given values:
P1 = 2.90 atm
T1 = -14°C = 259 K (converting to Kelvin)
T2 = 53°C = 326 K (converting to Kelvin)
(P1/T1) = (P2/T2)
(2.90 atm / 259 K) = (P2 / 326 K)
Solving for P2:
P2 = (2.90 atm / 259 K) * 326 K
P2 = 3.64 atm
Therefore, the final pressure when the temperature is 53°C is 3.64 atm.
A gas sample has a pressure of 2.90 atm when the temperature is - 14 deg C What is the final pressure, in atmospheres, when the temperature is 53 deg C with no change in the volume or amount of xpress your answer with the appropriate units
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