posted by Chelsey
A sample of gas at a temperature of 37.0°C has a pressure of 725 torr and occupies a volume of 3.44 L.
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.
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.
c. Use Charles’ law to calculate the new volume if the pressure is held constant and the temperature is increased to 210°C.
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.
e. Use the ideal gas law to calculate the number of moles of gas that are present.
725(3.44)=?(6.54) = 381.45
725(6.00)/37.0. = 117.567
725*3.44/37.0=?(16.9)/25.0 = 45.566
I keep getting b,c,d,e wrong but I don't know what I'm doing wrong
2 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)
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.