Question

Mg reacts with H+ (aq) according to Mg(s)+2H+(aq)\to Mg_2+(aq)+H_2(g) Suppose that 0.524 g of Mg is reacted with 60.o ml of 1.0 M H+(aq). Assume that

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asked 2021-02-14
Mg reacts with H+ (aq) according to
\(\displaystyle{M}{g{{\left({s}\right)}}}+{2}{H}+{\left({a}{q}\right)}\to{M}{g}_{{2}}+{\left({a}{q}\right)}+{H}_{{2}}{\left({g}\right)}\)
Suppose that 0.524 g of Mg is reacted with 60.o ml of 1.0 M H+(aq). Assume that the density of the H+ (aq) solution os 1.00 g/ml,and that its specific heat capacity equals that of water. Theinitial and final temperatures are 22.0 degree celsius and 65.8degree celsius.
a) Is the reaction endothermic or exothermic?
b) Calculate \(\displaystyle\triangle{H}\) of of th reaction. Use correct sigs andgive units.
c) Calculate the \(\displaystyle\triangle{H}\) of the reaction per mole of magnesium.

Expert Answers (1)

2021-02-16
\(\displaystyle{M}{g{{\left({s}\right)}}}+{2}{H}^{+}{\left({a}{q}\right)}\to{M}{{g}^{{{2}+}}{\left({a}{q}\right)}}+{H}_{{2}}{\left({g}\right)}\)
Part a)
Reaction of Metallic magnesium with acid is an exothermic reaction
Part b)
We have, Moles of \(\displaystyle{M}{g}={\frac{{\text{Mass}}}{{\text{Molar mass}}}}={\frac{{{0.524}}}{{{24.305}}}}={0.02156}\ {m}{o}{l}\)
Now, mass of the solution = Mass of water + Mass of Mg = 0.524 + 60.0 = 60.524 g
\(\displaystyle{q}=-{m}{c}\triangle{T}\)
Where q is the heat released
c is the specific heat
\(\displaystyle\triangle{T}\) is the temperature change
Therefore, \(\displaystyle{q}={60.524}\times{4.184}\times{\left({65.8}-{22.0}\right)}=-{11091.6}\ {J}=-{11.09}\ {K}{J}\)
Part c)
Heat released per mole of \(\displaystyle{M}{g}={\left({\frac{{-{11091.6}}}{{{0.02156}}}}\right)}=-{514}{K}\frac{{J}}{{m}}{o}{l}\)
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