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April 1, 2015

April 1, 2015

Posted by **Chelsey** on Wednesday, February 26, 2014 at 6:46pm.

a. Use Boyle’s law to calculate the new pressure if the temperature is held constant and the volume is increased to 6.54 L.

torr

b. Use Gay-Lussac’s law to calculate the new pressure if the volume is held constant and the temperature is decreased to 6.00°C.

torr

c. Use Charles’ law to calculate the new volume if the pressure is held constant and the temperature is increased to 210°C.

L

d. Use the combined gas law to calculate the new pressure if the temperature is decreased to 25.0°C and the volume is increased to 16.9 L.

torr

e. Use the ideal gas law to calculate the number of moles of gas that are present.

Moles

A= p1v1=p2v2

725(3.44)=?(6.54) = 381.45

B. p1t1=p2/t2

725(6.00)/37.0. = 117.567

C= v1t1=v2t2

3.44(210)/37.0= 19.524

D= p1v1t1=p2v2t2

725*3.44/37.0=?(16.9)/25.0 = 45.566

E..?

I keep getting b,c,d,e wrong but I don't know what I'm doing wrong

- Chemistry help! -
**DrBob222**, Wednesday, February 26, 2014 at 9:46pm2 errors on B

1. should be p1/t1 = p2/t2

2. T must be in kelvin and you used C

3. Ans is about 652.

(725/310) = (p2/279)

C.wrong formula.

v1/t1 = v2/t2

(3.44/310) = v2/210)

Ans is approx 2.3 L

d.formula is (p1v1/t1) = (p2v2/t2)

(725*3.44/310) = p2*16.9/298).

Ans is approx 142.

e. PV = nRT

725*3.44 = n*0.0821*310

Solve for n.

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