8.The hydrogen-filled dirigible Hindenburg had a volume of 1.99×108L. If the hyd

Question

8.The hydrogen-filled dirigible Hindenburg had a volume of 1.99×108L.  

If the hydrogen used was produced by the reaction of carbon with steam, how many kilograms of carbon would have been needed to produce enough hydrogen to fill the dirigible at 23 ?C and 750 mm Hg pressure?
C(s)+H2O(g)?CO(g)+H2(g)

Titanium hydride, TiH2, has a density of 3.75 g/cm3.

Part B. Compare it with that in liquid H2 (0.070 g/cm3). Express your answer using two significant figures.

Part C.  How many cubic centimeters of H2 at STP are absorbed in making 1.20 cm3 of TiH2? Express your answer using two significant figures.

10.How many liters of O2 gas at 25 ?C and 0.970 atm pressure can be obtained by the catalytic decomposition of 22.8 g of hydrogen peroxide?

Titanium hydride, TiH2, has a density of 3.75 g/cm3.

Part B. Compare it with that in liquid H2 (0.070 g/cm3). Express your answer using two significant figures.

Part C.  How many cubic centimeters of H2 at STP are absorbed in making 1.20 cm3 of TiH2? Express your answer using two significant figures.

10.How many liters of O2 gas at 25 ?C and 0.970 atm pressure can be obtained by the catalytic decomposition of 22.8 g of hydrogen peroxide?

Explanation / Answer

8.

P = 750 mmHg = 750 / 760 atm = 0.987 atm

T = 273.15 + 23 = 296.15 K

R = 0.0821 L.atm.K-1.mol-1

V = 1.99 * 108 L

Ideal gas equation,

P V = n R T

n = 0.987 * 1.99 * 108 / (0.0821 * 296.15)

n = 8.08 * 106 mol of H2 gas is produced.

From the balanced equation,

1 mol of H2 is produced from 1 mol of C

Then,

8.08 * 106 mol of H2 is produced from 8.08 * 106 mol of C

Mass of C = moles * molar mass = 8.08 * 106 * 12.0 = 9.69 * 107 g. = 9.69 * 104 kg. of C is needed.

So,

9.69 * 104 kg. of carbon is needed.

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