A balloon is filled with H2 gas to a volume of 1610.2 mL. The pressure of the gas in the balloo

step 1 In this problem, 59 we have to consider a balloon filled with hydrogen gas. And let me mention t

A balloon is filled with H2 gas to a volume of 1610.2 mL....

A balloon is filled with $\mathrm{H}_{2}$ gas to a volume of $1610.2 \mathrm{~mL}$. The pressure of the gas in the balloon is $745.4 \mathrm{~mm} \mathrm{Hg}$, and the temperature is $22.7{ }^{\circ} \mathrm{C}$. What is the mass in grams of the $\mathrm{H}_{2}$ in the balloon?

Key Concepts

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. It is expressed as PV = nRT, where P represents pressure, V is volume, n stands for the number of moles, R is the gas constant, and T is the temperature in Kelvin. This law allows us to calculate any one property of a gas if the others are known, making it essential for solving problems involving gases under various conditions.

Temperature Conversion

Temperature conversion is the process of converting temperatures from one scale to another, notably from degrees Celsius to Kelvin when using the Ideal Gas Law. Since the gas constant R is defined using Kelvin, it is necessary to convert any Celsius temperature to Kelvin by adding 273.15. This conversion ensures that the temperature used in calculations is in the correct unit and accurately reflects the thermal energy of the gas.

Unit Conversion Techniques

Unit conversion techniques involve changing units of measurements to ensure consistency across all quantities in a calculation. In gas law problems, this can include converting volumes from milliliters to liters, pressure from mm Hg (or torr) to atmospheres, or other necessary conversions. Mastery of unit conversions is critical for the correct application of the Ideal Gas Law and other equations in science.

Molar Mass

Molar mass is the mass of one mole of a substance and is a crucial parameter for converting between moles and grams. In gas problems, once the number of moles is determined using the Ideal Gas Law, the molar mass is used to calculate the mass of the gas present. For diatomic molecules like hydrogen (H2), knowing the molar mass allows one to directly relate the moles of the gas to its mass in grams.

Transcript

Please give Ace some feedback