50 g of aluminum is reacted excess sulfuric acid, what volume of hydrogen is pro

Question

50 g of aluminum is reacted excess sulfuric acid, what volume of hydrogen is produced at 20 degree C and 785 torr? 2 Al(s) + 3 H_2SO_4 (aq) rightarrow Al_2(SO_4)_3(aq) + 3 H_2(g) It takes 110 seconds for a sample of carbon dioxide (CO_2) to effuse through a porous plug and 275 seconds for the same volume of an unknown gas to effuse under the same conditions. What is the molar the unknown gas (in g/mol)? Calculate the rate of effusion of NO_2 compared to SO_2 at the same temperature and pressure. Compare the root-mean-square speed of methane (CH_4) and Oxygen (O_2) at 20 degree C

Explanation / Answer

Balanced equation:
2 Al + 3 H2SO4 ===> Al2(SO4)3 + 3 H2

50 gm aluminium = 50 / 26.98 = 1.853 Moles

No of Moles of H2 to be produced = 1.853 x 3 /2 = 2.779 Moles

Let us calculate the volume of H2 gas for 2.779 Mole

PV = nRT

where:

P is the pressure of the gas = 785 torr = 1.03289

V is the volume of the gas

n is the amount of substance of gas (in moles) = 2.779 Mole

R is gas constant = = 0.0821 L atm K-1 Mol-1

T is the absolute temperature of the gas = 273 +20 = 293 K

substitute in the equation and calculate volume

V = 0.0821 x 2.779 x 293 / 1.03289

V = 64.72 Liter

Hence 64.72 liter of H2 will be produced at 20 Deg cel and 785 torr

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