A student must use 225 mL of hot water(cwater=4.184 J/g°C) in a lab procedure. Calculate theamount of heat required to raise the temperature of225 mL of water from 20.0 °C to 100.0 °C.

Answers

Answer 1

Answer:    q = 64 kJ

Explanation:

As you know, a substance's specific heat tells you how much heat is required to increase the temperature of  

1 g

of that sample by  

1

C

.

In water's case, you know that its specific heat is equal to  

4.18

J

g

C

. This tells you that in order to increase the temperature of  

1 g

of water by  

1

C

, you need to supply  

4.18 J

of heat.

How much heat would you need to increase the temperature of  

200 g

of water by  

1

C

?

Well, if you need  

4.18 J

per gram to increase its temperature by  

1

C

, it follows that you will need  

200

times more heat to get this done.

Likewise, if you were to increase the temperature of  

1 g

of water by  

76

C

, you'd need  

76

times more heat than when increasing the temperature of  

1 g

by  

1

C

.

Combine these two requirements and you get the total amount of heat required to increase the temperature of  

200 g

of water by  

76

C

.

Mathematically, this is expressed using the following equation

q

=

m

c

Δ

T

 

, where

q

- heat absorbed/lost

m

- the mass of the sample

c

- the specific heat of the substance

Δ

T

- the change in temperature, defined as final temperature minus initial temperature

Plug in your values to get

q

=

200

g

4.18

J

g

C

(

100

24

)

C

q

=

63536 J

I'll leave the answer rounded to two sig figs and expressed in kilojoules

q

=

64 kJ


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pls mark as brainliest

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Im not sure

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Answer:

0.32gcm3 .           I miss the old Kanye, straight from the 'Go Kanye

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Answer:

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Explanation:

Answer:

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Answers

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Explanation:

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Determine the moles in the given volume

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[tex]silver[/tex]

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Answers

Answer:

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Explanation:

is a chemical element with the symbol Ag (from the Latin argentum, derived from the Proto-Indo-European h₂erǵ: "shiny" or "white") and atomic number 47.

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Answers

Answer:

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