Question

Calculate each of the following quantities for an ideal gas.

a. Calculate the volume of the gas, in liters, if 1.75mol has a pressure of 0.990atm at a temperature of -4∘C.

b. Calculate the absolute temperature of the gas at which 3.13×10−3mol occupies 355. mL at 760. torr.

c. Calculate the pressure, in atmospheres, if 4.67×10−2mol occupies 412mL at 139∘C.

d. Calculate the quantity of gas, in moles, if 50.7L at 56.0∘C has a pressure of 11.25kPa .

Answer 1

PV=nRT. Make sure the units of R are consistent with the units you use.

Answer 2

For example, one value of R = 0.082058 L atm /(mol K). You will need to convert all of your temps into Kelvin.

Answer 3

PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = moles (in moles)
R = gas constant = 0.0821 L(atm)/mol(K)
T = temperature (in K)

Make the required convertions and plogin the values in the formula:

a. V = 39.0L
b. T = 1380K
c. Temp 139C +237 = 412K; P = 3.8atm
d. n=0.209mol

Answer 4

but please remember 760torr=1atm