How many grams of hydrogen are in a 46.5 L balloon at 18.5°C and standard pressure?

To determine the mass of hydrogen in a balloon, we need to use the Ideal Gas Law (PV = nRT), where P is the pressure, V is the volume, n is the number of moles of the gas, R is the gas constant and T is the temperature in Kelvin. Given that the pressure is at standard pressure (1 atm), the volume is 46.5L, and the temperature is 18.5°C (which is equivalent to 291.65K), we can solve for n, the number of moles. The gas constant R is 0.0821 L·atm/K·mol.

Plugging the given values into the Ideal Gas Law equation we have: 1 atm * 46.5 L = n * 0.0821 L·atm/K·mol * 291.65K. Solving for n, gives us approximately 1.956 moles.

Knowing that one mole of hydrogen gas (H2) weighs approximately 2 grams, we can calculate the mass of hydrogen in the balloon by multiplying the number of moles by the molar mass. So it is about 1.956 moles * 2 g/mol = 3.912 g.

Therefore, the mass of hydrogen gas in the balloon is approximately 3.912 grams.

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