An experiment shows that a 248-mL gas sample has a mass of 0.433 g at a pressure of 745 mmHg an

step 1 solution for the given question here here we have to determine the number of moles combining all

An experiment shows that a 248-mL gas sample has a mass of...

An experiment shows that a $248-\mathrm{mL}$ gas sample has a mass of $0.433 \mathrm{~g}$ at a pressure of $745 \mathrm{mmHg}$ and a temperature of $28^{\circ} \mathrm{C}$. What is the molar mass of the gas?

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Key Concepts

Molar Mass Calculation

Molar mass is a measure of the mass of one mole of a substance. In the context of a gas, it is determined by first calculating the number of moles using the Ideal Gas Law and then dividing the mass of the gas sample by the number of moles. This calculation links experimental measurements with a fundamental property of the substance.

Unit Conversion

Proper unit conversion is critical in gas law calculations because the Ideal Gas Law requires consistent units, typically using pressure in atmospheres, volume in liters, and temperature in Kelvin. Converting all given measurements to the appropriate units ensures the accuracy of the calculations and the resulting molar mass determination.

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry and physics that relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law provides a framework for understanding how gases behave under different conditions and is essential for calculations involving gas properties.

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