in this lab you will be calculating $delta_{r}h$ for several chemical reactions using the technique of constant - pressure calorimetry. you will be monitoring the temperature of the water inside the test tube and then computing reaction $delta_{r}h$ values afterwards.
in every experiment, the temperature shown on the thermometer will increase during the reaction. this means every $delta_{r}h$ you report in this lab must be:
select one:
zero
positive
negative, because an increase in temperature means the reaction is exothermic

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# Brief Explanations:
In thermochemistry, for an exothermic reaction, heat is released. In constant - pressure calorimetry, when the temperature of the surroundings (here, the water) increases, it indicates that the reaction is exothermic. The enthalpy change of reaction $\Delta_{r}H$ is defined as $H_{products}-H_{reactants}$. For an exothermic reaction, $H_{products}<H_{reactants}$, so $\Delta_{r}H<0$ (negative). A positive $\Delta_{r}H$ would mean an endothermic reaction (heat absorbed, temperature of surroundings would decrease). A $\Delta_{r}H = 0$ would mean no heat exchange (not the case here as temperature is changing).
# Answer:
Negative, because an increase in temperature means the reaction is exothermic.

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