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3 years ago

6

If it takes 526 J of energy to warm 7.40g of water by 17 degrees celsius, how much energy would be needed to warm 7.40g of water

by 55 degrees celsius?

2 answers:

Shkiper50 [21]3 years ago

8 0

The energy needed to warm water be 55 Celsius would be
Q=m*c* Delta T

We are given the following data
Q=526
m=7.4
T=17C= 526/17*7.4

Putting in the equation we get

Q=mc DeltaT

<span>Q=7.4x55x526/17x7.4

=55x526/17
</span>
=1701.64 C

tester [92]3 years ago

5 0

Answer:

Heat required = 1702 J

Explanation:

The amount of heat energy (Q) required to raise the temperature of water of mass (m) is given as:

$Q = mc\Delta T$

where c = specific heat capacity

ΔT =change in temperature

It is given that:

When ΔT = 17 C, Q = 526 J and m = 7.40 g

i.e. $526J = 7.40g*c*(17 C) \\\\c = 4.181 J/g C$

The amount of heat required to increase the temperature of 7.40 g water by 55 C would be:

$Q = 7.40 g*4.181J/gC*55C =1702 J$

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