Equal volumes of propane, C_3H_s, and carbon monoxide al the same temperature an

Question

Equal volumes of propane, C_3H_s, and carbon monoxide al the same temperature and pressure have the same density. number of molecules. number of atoms. 1 only 2 only 3 only 1 and 2 only 1.2. and 3 2. The valve between the 2.00-L bulb, in which the gas pressure is 1.00 atm, and the 3.00-L bulb, in which the gas pressure is 1.50 atm. is opened What is the final pressure in the two bulbs, the temperature remaining constant? 0.900 atm 1.25 atm 1.30 atm 2.25 atm 2.50 atm The volume of a sample of gas measured at 25.0 degree C and 1.00 atm pressure is 10.0 L. What must the final temperature be in order for the gas to have a final volume of 7.5 L at 1 00 atm pressure? -55 degree C -50 degree C -45 degree C -35 degree C 19 degree C

Explanation / Answer

1)

we know that

PV = nRT

given

P , V and T are same for all

so

they should have same number of moles

same number of moles means same number of molecules

now

density = mass / volume

mass = moles x molar mass

so

density = moles x molar mass / volume

in this case

moles and volume are same for all

but their molar masses are different

so

density is different for all

the answer is

b) 2 only

2)

when the value opens

eveything changes but mass remains same

so

n = n1 + n2

we know that

moles (n) = PV / RT

so

PV/RT = (P1V1/RT) + (P2V2/RT)

now

Temp (T) and R are constant

so

PV = P1V1 + P2V2

so

P x 5 = (2 x 1) + ( 1.5 x 3)

P = 1.3

so

the final pressure is 1.3 atm

answer is c) 1.3 atm

3)

we know that

PV / T = constant

so

P1V1/T1 = P2V2/T2

given

P1 = 1

V1 = 10

T1 = 298 K

P2 = 1

V2 = 7.5

so

1 x 10 / 298 = 1 x 7.5 / T2

T2 = 223.5 K

T2 = 223.5 - 273

T2 = -49.5 C

so

the answer is b) -50 C

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