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uranmaximum [27]
3 years ago
8

How many calories is required to change the temperature of 2.18g of water from 15.3°C to 69.5°C. The specific heat of liquid wat

er is 1.00cal/g°C.
Chemistry
2 answers:
lozanna [386]3 years ago
7 0

The number  of calories that are  required  to change the temperature  of 2.18 g of water from 15.3 c to 69.5 c is  <u>118.16 cal</u>


    <u><em> calculation</em></u>

  •    Heat in calories  = MCΔ T where,
  • M(mass)= 2.18 g
  • C(specific heat capacity)= 1.00 cal/g/c
  • ΔT( change in temperature)= 69.5- 15.3 =54.2 c

 heat is therefore= 2.18 g x 1.00 cal/g/c  x 54.2 c=118.16  cal

kotykmax [81]3 years ago
5 0

<u>Given:</u>

Mass of water, m = 2.18 g

Initial temperature of water, T1 = 15.3 C

Final temperature, T2 = 69.5 C

Specific heat, c = 1.00 cal/gC

<u>To determine:</u>

Heat required to raise the water temperature

<u>Explanation:</u>

The amount of heat, Q, required to raise the temperature of water from T1 to T2 is:

Q = mcΔT = mc(T2-T1)

Q = 2.18 * 1 * (69.5-15.3) = 118.16 cal

Ans: Heat required is 118.16 cal

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