Question

A 0.250-g sample of a magnesium-aluminum alloy dissolves completely in an excess of HCl(aq). When the liberated H2(g) is collected over water at 29 ∘C and 752 torr, the volume is found to be 325 mL . The vapor pressure of water at 29 ∘C is 30.0 torr.

How many moles of H2 can be produced from *x* grams of Mg
in magnesium-aluminum alloy? The molar mass of Mg is 24.31
g/mol.

Express your answer in terms of *x* to four decimal
places (i.e., 0.5000x).

How many moles of H2 can be produced from *y* grams of Al
in magnesium-aluminum alloy? The molar mass of Al is 26.98
g/mol.

Express your answer in terms of *y* to four decimal
places (i.e., 0.5000y).

Answer #1

No. of moles of H2 is 0.0132

The equations of reaction are:

Mg +2 HCl --> MgCl2 + H2

2 Al + 6 HCl --> 2 AlCl3 + 3 H2

Atomic mass of Mg is 24.31 g/mol and of Al = 26.98 g/mol.

If all of the alloy was Al, we have to calculate the mass of Al =
2/3*mol[H2]*26.98 g/mol = 237.4240 mg

If it all was Mg we calculate mol[H2]*24.31= 320.8920 mg

If Al is 85.5 % and Mg 14.5 % the alloy produces the amount of H2
given.

At first we have to calculate the gas volume at standard condition (25°C and 760 torr)

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