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ZanzabumX [31]
3 years ago
12

A large flask is evacuated and weighed, filled with argon gas, and then reweighed. When reweighed, the flask is found to have ga

ined 3.221 g. It is again evacuated and then filled with a gas of unknown molar mass. When reweighed, the flask is found to have gained 8.107 g. Part A To estimate the molar mass of the unknown gas based on the molar mass of argon, which assumptions should be made?
Chemistry
1 answer:
vivado [14]3 years ago
8 0

Answer:

The molar mass of the unknown gas is 100.4 g/mol

Explanation:

Step 1: Data given

Molar mass of argon = 39.95 g/mol

After filling with argon the flask gained 3.221 grams

After filling with an unknown gas, the flask gained 8.107 grams

Step 2: Calculate the molar mass of the unknown gas

The gas with the higher molar mass will have the higher density.

Ar - 3.224 g; molar mass = 39.95 g/mol

X = 8.102 g; molar mass = ??

Molar mass of the unknown gas = 8.102g X *(39.95 g/mol  / 3.224 g) = 100.4 g/mol

The molar mass of the unknown gas is 100.4 g/mol

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First I had to look for the problem to know the possible answers.

In this case, the coffee jug has a large amount of coffee at the same temperature. If we analyze that the decanter and the coffee are at the same temperature, we have a homogeneous thermal system. The cup is at room temperature, so by pouring coffee into it, the temperature of the coffee decreases to balance with the temperature of the cup. At this moment, the temperature of the cup-cafe system is lower than the jug-cafe system.

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