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A 2.62g sample of a substance suspected of being pure gold is warmed to 72.3∘C and submerged into 15.6g of water initially at 24.8∘C. The final temperature of the mixture is 26.0∘C. What is the heat capacity of the unknown substance?

Respuesta :

Answer:

specific heat capacity of the unknown is 629.66 J/kg C

Explanation:

As we know that gold is heated to 72.3 degree C and mixed with water at 24.8 degree C

Now the final temperature of the mixture is 26 degree C

here we can say that heat given by the gold = heat absorbed by the water

So we will have

[tex]Q_{in} = Q_{out}[/tex]

[tex]2.62 s (72.3 - 24.8) = 15.6 (4186) (26 - 24.8)[/tex]

so we will have

[tex]s = 629.66 J/kg C[/tex]

so specific heat capacity of the unknown is 629.66 J/kg C

Specific heat capacity of the unknown is 629.66 J/kg C

Given that,

  • A 2.62g sample of a substance suspected of being pure gold is warmed to 72.3∘C and submerged into 15.6g of water initially at 24.8∘C.
  • The final temperature of the mixture is 26.0∘C.

Calculation of heat capacity:

= 2.62s (72.3 - 24.8)

= 15.6 (4186)  (26 - 24.8)

s = 629.66

Find out more information about the temperature here: https://brainly.com/question/7510619?referrer=searchResults

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