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nadya68 [22]
4 years ago
11

A sample of gas has a pressure of 3.00 atm at 25 degrees Celsius. What would the pressure be at 52 degrees Celsius if the volume

stays constant? Which gas law does this problem represent?
Chemistry
1 answer:
Doss [256]4 years ago
8 0
The law that relate pressure and temperature of gases at constant volumes is Gay-Lussac's Law.

It states that the pressure of a fixed mass of gas is directly proportional to the absolute temperature when the volume is constant.

 P / T = constant => P1 / T1 = P2 / T2

=> P2 = T2 * P1 / T1

Remember that the formula uses absolute temperatures.

T2 = 52 + 273.15 = 325.15 K

T1 = 25 + 273.15 = 298.15 K

=> P2 = 325.15K * 3.00 atm / 298.15K = 3.27 atm.

Answer: 3.27 atm
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P_2=1.48atm

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to infer this problem is about the application of the Gay-Lussac's gas law to relate the initial and final pressure and temperature as shown below:

\frac{P_2}{T_2} =\frac{P_1}{T_1\\ }

Thus, solving for the final pressure, P2, and using the temperatures in Kelvins, we obtain:

P_2 =\frac{P_1T_2}{T_1 }\\\\P_2 =\frac{1atm*403.15K}{273.15K}\\\\P_2=1.48atm

Regards!

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0.00632 into a scientific notation
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