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OleMash [197]
3 years ago
11

Calculate the approximate enthalpy of the reaction in joules. Estimate that 1.0 mL of vinegar has the same thermal mass as 1.0 m

L of water. It takes 4.2 joules to change 1.0 grm (1.0 mL) of water 1.0 Celcius. Is it endotherrmic or exothermic? Volume of vinegar 25 mL, Initial temp of vinegar 17 Celcius and final temp is 14 Celcius.
Chemistry
1 answer:
Nesterboy [21]3 years ago
5 0

Explanation:

The given data is as follows.

   Density of vinegar = 1.0 g/ml

   Specific heat capacity = 4.25 J/g ^{o}C

   T_{1} = 17 ^{o}C,  and   T_{2} = 14 ^{o}C

Relation between enthalpy and specific heat is as follows.

                   \Delta H = mC \Delta T

Hence, putting the values into the above formula as follows.

          \Delta H = mC \Delta T

                  = 25 \times 1.0 \times 4.25 J/g ^{o}C \times -3^{o}C          (as density = \frac{mass}{volume})

                               = - 315 J

Thus, we can conclude that the enthalpy of reaction is -315 J.

As the value is negative so, it means that heat is releasing. Hence, the reaction is exothermic in nature.

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There's is no further explanation for this.

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Electrons in the 3d sublevel, are found mostly in all the transition metals of period 3, and it can go from 1 to 10 electrons. To be with the 3d sub level it's neccesary that the energy level to be 3.

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Answer:

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Hello there!

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Thus, since we are interested in the initial temperature, we can solve for T1, plug in the volumes and use T2 in kelvins:

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