# What would be the effect on the calibration factor obtained from an experiment if you used 50mL water instead of 100 mL of water to calibrate the calorimeter?

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The calibration factor `F` of a calorimeter is by definition to the heat supplied to the calorimeter divided by the temperature change.

To determine the value of ` ` the calorimeter you heat a known mass of water in the calorimeter from an initial temperature to a final temperature with a known heat `Q` provided by an electric heater supplied with a known voltage and current.

Thus if `C` is the heat capacity of the calorimeter itself:

`Q =C*Delta(T) +m*c_(water)*Delta(T)`

The calibration factor is

`F = Q/(Delta(T)) (=(U*I*t)/(Delta(T))) = C +m*c_(water)`

`F =C +m*c_(water)`

Usually a calorimeter is made of a metal and has small mass. Thus the value of calorimeter heat capacity `C` is about ten times smaller than the heat capacity of water inside it, `m*c_("water")` . Hence the above relation can be approximated well with

`F ~~m*c_("water")`

Now we have the answer: **if we use half of initial mass of water to calibrate the calorimeter the calibration factor will be reduced to about half of its initial value.**

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