Question

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?

Answer 1

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 

Q=7.4x55x526/17x7.4

=55x526/17

=1701.64 C

Answer 2

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:

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