The 200-mm test tube also contained some water (besides the metal) that was subsequently added to the calorimeter (in Part A.4.). Considering a higher specific heat for water, will the temperature change in the calorimeter be higher, lower, or unaffected by this technique error?

The temperature  change in the calorimeter will be lower

Explanation:

Water is an example of a molecular substance. They have relatively low melting points and boiling points usually below 300° C . Water reacts with metals to a degree varying with their position in the electrochemical series.

The specific heat of water is 4179.6 Joules which is relatively high . This typically implies that water absorbs a larger amount of heat but the increase in temperature of its boiling points is relatively low. Thus; in the 200-mm test tube that contains water and was subsequently added to the calorimeter , the heat present was initially absorbed by the water and that does not result to an increase in the temperature change in the calorimeter. Thus the temperature change in the calorimeter will be lower.

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