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3 years ago

If we read the reaction as X + Y → Z + Q it is A. endothermic B. exothermic

Chemistry

2 answers:

Korvikt [17]3 years ago

4 0

As you can see in the picture we have +ΔH so that means for this reaction we need to GET heat. so the answer is A. endothermic :))
i hope this is helpful
have a nice day

kupik [55]3 years ago

3 0

Answer: The given reaction is a type of endothermic reaction.

Explanation:

There are 2 types of reaction classified on the basis of heat released or absorbed:

1. Exothermic reactions: In these reactions, the heat is released because the energy of products is less than the energy of the reactants. $\Delta H$ for these reactions is negative.

2. Endothermic reactions: In these reactions, heat is absorbed by the reactants because the energy of the products is more than the energy of the reactants. $\Delta H$ for these reactions if positive.

In the given question, the energy of the products is greater than the energy of the reactants. Hence, this is considered as a type of endothermic reaction.

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Answer : The heat of combustion per mole of caffeine at constant volume is 76197.18 kJ/mole

Explanation :

First we have to calculate the specific heat calorimeter.

Formula used :

$Q=m\times c\times \Delta T$

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Q = heat of combustion of benzoic acid = 26.38 kJ/g = 26380 J/g

m = mass of benzoic acid = 0.235 g

c = specific heat of calorimeter = ?

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Now put all the given value in the above formula, we get:

$26380J/g=0.235g\times c\times 1.643^oC$

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Thus, the specific heat of calorimeter is $68323.38J/^oC$

Now we have to calculate the heat of combustion of caffeine.

Formula used :

$Q=c\times \Delta T$

where,

Q = heat of combustion of caffeine = ?

c = specific heat of calorimeter = $68323.38J/^oC$

$\Delta T$ = change in temperature = $1.584^oC$

Now put all the given value in the above formula, we get:

$Q=68323.38J/^oC\times 1.584^oC$

$Q=108224.23J=108.2kJ$

Now we have to calculate the moles of caffeine.

$\text{Moles of caffeine}=\frac{\text{Mass of caffeine}}{\text{Molar mass of caffeine}}$

Mass of caffeine = 0.275 g

Molar mass of caffeine = 194.19 g/mole

$\text{Moles of caffeine}=\frac{0.275g}{194.19g/mole}=0.00142mol$

Now we have to calculate the heat of combustion per mole of caffeine at constant volume.

$\text{Heat of combustion per mole of caffeine}=\frac{108.2kJ}{0.00142mol}=76197.18kJ/mole$

Therefore, the heat of combustion per mole of caffeine at constant volume is 76197.18 kJ/mole

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3 years ago

At a pressure of 1.00 atm, the solubility of nitrogen in water is 23.5 mg gas/100 g water. Indicate whether each of the followin

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Answer:

a) Solubility diminishes.

b) Solubility remains constant.

c) Solubility increases.

d) Solubility increases.

Explanation:

Hello,

a) In this case, we've got to take into account that the solubility of a gas into a liquid increases as the pressure does it (because the molecules are forced to gather with the liquid's particles) and the other way around, in such a way, as the pressure is decreased, the solubility is decreased as well.

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c) Now, as the pressure is increased, the solubility is increased in a very similar way that in the a) part.

d) Submerging the solution 40m underwater means that the fluid's column above the solution is increased, thus, the pressure is increased, so the solubility is increased as well.

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