🤓 Based on our data, we think this question is relevant for Professor DeSimone's class at UA.
Initially, a gas sample has a volume of 859 mL at 565 K and 2.20 atm. We’re being asked to determine the pressure of the gas sample if the volume changes to 268 mL and the temperature changes to 815 K.
Recall that the ideal gas law is:
The pressure, volume, and temperature of a gas are related to the number of moles of gas and the universal gas constant:
The value nR is constant. For a given moles of gas, the initial and final pressure, volume, and temperature of the gas are related by the combined gas law:
A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What is the pressure of the sample if the volume changes to 268 mL while the temperature is increased to 815 K?
A. 9.83 atm
B. 1.05 atm
C. 15.3 atm
D. 6.53 atm
E. 10.2 atm
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Our tutors have indicated that to solve this problem you will need to apply the Chemistry Gas Laws concept. If you need more Chemistry Gas Laws practice, you can also practice Chemistry Gas Laws practice problems.
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Based on our data, we think this problem is relevant for Professor DeSimone's class at UA.