Asample of an unknown compound is vaporized at 190.°c. the gas produced has a volume of 2420.ml at a pressure of 1.00 atm, and it weighs 2.04 g. assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. be sure your answer has the correct number of significant digits.

Answer : The molar mass of unknown compound is, 32.0 g/mole

Explanation :

Using ideal gas equation:

where,

P = pressure of gas = 1.00 atm

V = volume of gas = 2420 ml = 2.420 L      (1 L = 1000 ml)

T = temperature of gas =

n = number of moles of gas

R = gas constant = 0.0821 L.atm/mole.K

w = mass of unknown compound = 2.04 g

M = molar mass of unknown compound = ?

Now put all the given values in the ideal gas equation, we get:

Therefore, the molar mass of the compound is, 32.0 g/mole

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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