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AlexFokin [52]
3 years ago
12

31.5 grams of an unknown substance is heated to 102.4 degrees Celsius and then placed into a calorimeter containing 103.5 grams

of water at 24.5 degrees Celsius. If the final temperature reached in the calorimeter is 32.5 degrees Celsius, what is the specific heat of the unknown substance?
Show or explain the work needed to solve this problem, and remember that the specific heat capacity of water is 4.18 J/(°C x g). (2 points)
Chemistry
1 answer:
Alexxandr [17]3 years ago
5 0
Heat gained in a system can be calculated by multiplying the given mass to the specific heat capacity of the substance and the temperature difference. It is expressed as follows:<span>

Heat = mC(T2-T1) 

When two objects are in contact, it should be that the heat lost is equal to what is gained by the other. From this, we can calculate things. We do as follows:

</span>Heat gained = Heat lost
mC(T2-T1) = - mC(T2-T1) 
31.5C (102.4 - 32.5) = 103.5(4.18)(32.5 - 24.5)
C = 1.57 J/C-g

Hope this helps.
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Arun and Marcus are asked to compare the solubility of two salts in water at room temperature. The two salts are labelled X and
oksian1 [2.3K]

Answer:

1) Salts X and Y

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3) a) The solvent

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Explanation:

1) The independent variable is the variable that is suspected to be the cause of the subject of the investigation

The given investigation is meant to investigate the solubility of different salts

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3 0
3 years ago
How many atoms are in 1.204x10^22 moles of arsenic?
ra1l [238]

Answer:

<h2>0.02 moles </h2>

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n =  \frac{N}{L} \\

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N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

We have

n =  \frac{1.204 \times  {10}^{22} }{6.02 \times  {10}^{23} }    \\  = 0.02

We have the final answer as

<h3>0.02 moles</h3>

Hope this helps you

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