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