Astrip of magnesium metal having a mass of 1.30 g dissolves in 150. ml of 5.00 m hcl (specific gravity = 1.10); products of the reaction are magnesium chloride and hydrogen gas. the hcl is initially at 22.0°c, and the resulting solution reaches a final temperature of 52.0°c. the heat capacity of the calorimeter in which the reaction occurs is 345 j/°c. calculate δh (in kj/mol) for the reaction under the conditions of the experiment, assuming the specific heat of the final solution is the same as that for water (4.184 j/g°c).
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Ответ:
Explanation:
The given data is as follows.
Mass of Mg = 1.30 g, Molarity = 5 for HCl, Volume = 150 mL
Density = 1.1 g/mL
Change in temperature (dT) =![(52 - 22)^{o}C = 30^{o}C](/tpl/images/0291/7543/add13.png)
Hence, the energy balance will be as follows.
Moles of Mg =![\frac{mass}{\text{molecular mass}}](/tpl/images/0291/7543/39dc1.png)
=![{1.3}{24.3}](/tpl/images/0291/7543/04f08.png)
= 0.05349 mol of Mg
=![345 J/^{o}C \times 30^{o}C](/tpl/images/0291/7543/a4309.png)
= 10350 J
=![150 \times 1.1 \times 4.184 \times 30^{o}C](/tpl/images/0291/7543/61f7c.png)
= 20710.8
Therefore, calculate the value of
of the reaction as follows.
or,
(as 1 kJ = 1000 J)
Thus, we can conclude that value of
of the reaction under given conditions is -580.68 kJ/mol.
Ответ:
it’s C
Explanation:
A distant luminous object travels rapidly away from an observer.