A 1.00 mol sample of gas at 25C and 1.0 atm has an initial volume of 22.4L. Calc

LoidaSanchez

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10 years ago

A 1.00 mol sample of gas at 25C and 1.0 atm has an initial volume of 22.4L. Calc

A 1.00 mol sample of gas at 25 degrees Celcius and 1.0 atm has an initial volume of 22.4L. Calculate the result of each change, assuming all other conditions remain constant.

1. The pressure is changed to 85.7mmHg. How many mm does the gas occupy?
2. 2. The volume is reduced to 275 mL. What is the pressure in millimeters of mercury?

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Alexx

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10 years ago

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How many mm does the gas occupy?

You mean ml right?
We use the formula P*V=k where P is pressure, V is volume and k is constant.
1 atm= 760mmHg. At first we have k=760*22,4=17024mmHg*L
And then, we have: P1*V1=k <=> 85,7*V=17024 <=> V=198,65L=198650ml
B) we used Liters to calculate k so we need to make 275ml=0,275L
P2*V2=k <=> P2*0,275=17024 P2=61905,4545...mmHg

Mercury is hydrargyrum. Interesting!

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LoidaSanchez Author

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10 years ago

Yes i meant ml thank you could you explain that because on my sheet it only has the answers as : 1.99 × 10to the 5 mL , 6.19 × 10to the 4 mmHg

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Alexx

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10 years ago

1.99*105=199000ml, which is a rounding of the number 198650ml

6.19*104=61900mmHg, which is a rounding of the number 61905,4545mmHg.

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could you explain that

To solve the problem I used the Boyle's law. According to Boyle's law, when I have a certain quantity of gas, and fixed temperature, then the values of pressure and volume can be described with the equation: PV=k, where P is pressure, V is volume, and k is a constnat.
http://en.wikipedia.org/wiki/Boyle%27s_law

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