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r-ruslan [8.4K]
3 years ago
6

The temperature of 335 g of water changed from 24.5oC to 26.4oC. How much heat did this sample absorb? C for water = 4.18 J/goC

Chemistry
1 answer:
Sergio039 [100]3 years ago
8 0

Answer: The sample absorbed 3061.565J

Explanation:

Given that  

Mass of water  = 335g

Initial temperature  = 24.5°C

Final temperature = 26.4°C

Heat  absorbed by the sample is given as  = mass x specific heat of water x  temperature change

Heat  absorbed,q=mCΔt

The specific heat of water,C  = 4.81J/g°C

 

Therefore,  Heat absorbed,q  = 335 x 4.81h x (26.4  - 24.5)  = 3061.565J

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Answer:

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Making V the subject of the above equation, we have:

PV = nRT

Divide both side by P

V = nRT / P

Thus, we can say that the volume (V) is directly proportional to both the number of mole (n) and absolute temperature (T) and inversely proportional to the pressure (P). This implies that and increase in either the number of mole, the absolute temperature and a decrease in the presence will cause the volume to increase.

Thus, the correct option is option C triple the number of moles. This can further be seen as illustrated below:

Initial volume (V1) = 12 L

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Final mole (n2) = triple the initial mole = 3 × 0.5 = 1.5 mole

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From:

V = nRT / P, keeping T and P constant, we have:

V1/n1 = V2/n2

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24 = V2/1.5

Cross multiply

V2 = 24 × 1.5

V2 = 36 L.

Thus Option C gives the correct answer to the question.

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