A balloon is filled with hydrogen gas. reaction is Fe(s) + H2SO4(aq) ----> FeSO4(aq) + H2(g).

The volume of the ballon was 4800 m cubed and the loss of hydrogen gas during filling was estimated at 20.% What mass of iron splints and 98% by mass H2SO4 were needed to ensure the complete filling of the balloon? Assume a temperature of 0 degrees celsius, a pressure of 1.0 atm during filling, and a 100% yield.

4800 m^3 = 4.8E6 L but you should confirm that.

PV = nRT. T is 273 K. Substitute from the problem and solve for n = number of mols. Then add 20% (0.20) to that to make up for the 20% loss.
Convert mols H2 to mols Fe. 1 mol H2 requires 1 mol Fe according to the equation. Then g Fe = mols Fe x atomic mass Fe.

Convert mols H2 to mols H2SO4. 1 mol H2 requires 1 mol 100% H2SO4 according to the equation. Then grams H2SO4 = mols H2SO4 x molar mass H2SO4 if H2SO4 is 100%. It isn't so grams 100%H2SO4/0.98 = grams 98% H2SO4. Post your work if you get stuck.

Thanks

To find out the mass of iron splints and 98% by mass H2SO4 needed to ensure the complete filling of the balloon, we need to follow these steps:

1. Convert the volume of the balloon from cubic meters to liters:
4800 m^3 = 4800 x 1000 = 4,800,000 L

2. Calculate the volume of hydrogen gas that will be lost during filling:
Volume lost = 20% of 4,800,000 L = (20/100) x 4,800,000 = 960,000 L

3. Calculate the volume of hydrogen gas that will remain in the balloon after filling:
Volume remaining = Total volume - Volume lost
= 4,800,000 L - 960,000 L
= 3,840,000 L

4. Use the ideal gas equation to find the number of moles of H2 gas in the remaining volume:
PV = nRT (P = pressure, V = volume, n = moles, R = ideal gas constant, T = temperature)
n = PV / RT
Since the temperature is 0 degrees Celsius, which is 273.15K, and the pressure is given as 1.0 atm, we can plug in these values:
n = (1.0 atm) x (3,840,000 L) / [(0.0821 L.atm/mol.K) x (273.15K)]
n ≈ 175,861 moles

5. Now, according to the balanced chemical equation, the ratio between moles of Fe and moles of H2 is 1:1. Therefore, the number of moles of Fe needed is also approximately 175,861.

6. Calculate the molar mass of Fe(s) (iron) from the periodic table. It is approximately 55.85 g/mol.

7. Calculate the mass of iron needed:
Mass of Fe = Moles of Fe x Molar mass of Fe
= 175,861 moles x 55.85 g/mol
≈ 9,812,278 g or 9.81 kg

8. To find the mass of 98% H2SO4 needed, we need to calculate the mass percent of sulfuric acid in the mixture:
Mass percent of H2SO4 = 100% - 98% (as the remaining 2% can be considered as diluting substance)
= 2%

9. Calculate the mass of H2SO4 needed:
Mass of H2SO4 = Mass of mixture x Mass percent of H2SO4 / 100%
≈ 9.81 kg x 2% / 100%
≈ 0.1962 kg or 196.2 g

Therefore, to ensure the complete filling of the balloon, approximately 9.81 kg of iron splints and 196.2 g of 98% H2SO4 are needed.