Question

How many calories are absorbed when \[500grams\] of water \[\left( {1cal/gc} \right)\] is heated from \[50to100\] degrees Celsius?

Answer 1

Hint: All you require to know is the substance being heated, the change in temperature and the mass of the substance. The equation is:
\[Q = \] \[mc\vartriangle T\]
Here, Q implies heat, m is mass, c is specific heat capacity and ∆T is the change in temperature. You can discover the adjustment in temperature by taking away the beginning temperature from the last temperature.

Complete step by step answer:
You realize that the specific heat of a substance reveals to you the measure of heat expected to build the temperature of \[1g\] of that substance by{1^0}C.In your case, water is said to have a specific heat equivalent to
\[{C_{water}} = 1cal{g^{ - 1}}C\]
This implies that to expand the temperature of \[1g\] of water by{1^0}C, you need to provide it with \[1cal\] of heat. Thus, how much heat would be expected to expand the temperature of \[500grams\] of water by{1^0}C
500g \times \dfrac{{1cal}}{{1g}} = 500cal
This implies that to expand the temperature of \[500g\] of water by
${100^o}C - {50^0}C = {50^0}C$
you need to give it
${50^0}C \times \dfrac{{500cal}}{{{1^0}C}} = 25000cal$
The appropriate response should be adjusted to one significant figure, the number of sig figs you have for your values.

Note: This much heat is required to get \[500g\] of water from liquid at{50^0}C to liquid at{100^o}C
Heat capacity is the measurable physical amount that characterizes the measure of heat needed to change a substance's temperature by a given sum. It is measured in joules per Kelvin and given by.
The heat capacity is an extensive property, scaling with the size of the system.
The heat capacity of most systems is not constant (however it can regularly be treated as such). It depends on the temperature, pressure, and volume of the system consideration.