The new pressure of the gas would be 505.58 torr
<h3>Boyle's law</h3>
According to Boyle's law, the pressure of a gas is inversely proportional to its volume, provided that the temperature is constant.
This can be mathematically represented as: P1V1 = P2V2
In this case, P1 = 759.4 torr, P2 is what we are looking for, V1 = 97.6 mL, and V2 = 146.6 mL
Hence, P2 = P1V1/V2 = 759.4x97.6/146.6 = 505.58 torr
More on Boyle's law can be found here: brainly.com/question/1437490
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Answer:
7366.328 kPa.
Explanation:
- The critical pressure of carbon dioxide is 72.7 atm.
- To convert from atm to kPa, we use the relation that:
1.0 atm = 101.325 kPa.
- Applying conversion factor:
<em>The conversion factor = (101.325 kPa/1.0 atm)</em>
<em></em>
∴ The critical pressure of carbon dioxide (in kPa) = (72.7 atm)(101.325 kPa/1.0 atm) = 7366.328 kPa.
Answer:
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