1.When an evacuated 100.0 - mL glass bulb is filled with a gas at 22.0 degrees C

Question

1.When an evacuated 100.0 - mL glass bulb is filled with a gas at 22.0 degrees C and 747 mmHg. The bulb gains 0.1137 grams. Which gas is in the bulb, neon, argon, or nitrogen gas? Show proof by calculation.

2. A 355 mL steel container at 35.0 degrees C contains only Neon and Argon gases at a total pressure of 0.0824atm. If there is 0.145 grams of Neon in the container, how many grams of Argon is there?

(Extra question for max points)

Consider the following decompostion reaction of a cobalt compound in a vacuum:

Co2(CO)8 (s) --> 2Co (s) + 8CO (g)

If 0.245 grams of Co2(CO)8 is decomposed, and the carbon monoxide gas is trapped in a 500. mL flask at 150 degrees C, what will be the pressure of the collected gas?

Explanation / Answer

1) let the molar mass of the gas be x grams/mol .so,

using the ideal gas equation,

PV=nRT,

(747/760)*0.1=(0.1137/x)*0.0821*(273+22)

or x=28 grams/mol

so the gas is nitrogen since it's molecular mass is 28 grams/mol

2)let the mass of argon be x.

so using the ideal gas equation, PV=nRT,

0.355*0.824=(0.145/20 + x/40)*0.0821*(273+35)

or x=0.172 grams

3)moles of CO formed=8*(0.245/342)

=5.73*10^-3 moles

so using the ideal gas equation,

PV=nRT,

P*0.5=5.73*10^-3*0.0821*(273+150)

or P=0.379 atm

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