Asample of an unknown compound is vaporized at 170 c. the gas produced has a volume of 1980 ml at a pressure of 1 atm, and it weighs 5.17 gr. assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. round your answer to 3 significant digits.

The molar mass is 95.7 g/mol

Explanation:

As the vapor formed is showing ideal gas behavior, it will obey ideal gas law.

PV = nRT

Where

P = Pressure = 1 atm

V = volume = 1980 mL = 1.98 L

n = moles of gas

R = gas constant = 0.0821 L atm /mol K

T = Temperature = 170 °C = 170+273 = 443 K

Putting values

1 X 1.98 = n X 0.0821 X 443

n = moles = 0.054 mol

the relation between moles and molar mass and mass is:

Therefore

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explanation:

definition

                    entropy is a measure of the randomness or the extent of disorder of a chemical process.

                      enthalpy is a measure of the heat change of a reaction occurring at a constant pressure.

measurement units:

                        entropy is measured in joule per kelvin (jk⁻¹)   whereas enthalpy is measured in joule per mole (jmol⁻¹)

requirements:

                            entropy has no requirements or limits, and its change is measured by the division between the heat change of the chemical process and the temperature.

                              in contrast, enthalpy can only be related to the heat change of the reaction under standard conditions.