Do you have evidence from the lab that your calorimeter was not a perfect insulator? Assuming that heat was lost from the calorimeter, describe specifically how that would impact the data you recorded and then chase that change through the calculations to show how the error would impact the calculated enthalpy change for a particular reaction.

In the past, we have done this lab with roughly 50 mL each of each reactant solution, instead of 25 mL. Yet the Δ T determined experimentally were roughly the same. Explain why that is.

Each student will have slightly different volumes of reactants for each reaction. Yet the results obtained for ΔH1, ΔH2, and ΔH3 should be quite similar and would in fact be quite similar for any range of reactants combined within 25-50 mL, provided that each is accurately measured. Explain why this is the case.

A student misreads the volume of one of the solutions as 25.0 mL when in fact it was 35.0 mL. Step through the quantitative consequences of this error on the heat generated, the Δ T observed, the q calculated, and the Δ H calculated. (Clarification: Both solutions “should” be 25.0 mL or something close, and one of the volumes is accidentally 35.0 mL)

A student pours the reaction solutions into a still wet Styrofoam cup. Step through the quantitative consequences of this error on the heat generated, the Δ T observed, the q calculated, and the Δ H calculated.

Heat losses in a calorimeter will lower the value of enthalpy change, ΔH, for a particular reaction.
An error in the volume of one of the reacting solutions will increase the heat generated, the ΔT observed, the q calculated, and the calculated ΔH.
Using a wet Styrofoam cup will lower the heat generated, the ΔT observed, the q calculated, and the calculated ΔH.

What is a calorimeter?

A calorimeter is a laboratory apparatus used to measure heat changes that occur in a reaction.

A calorimeter works on the principle of conservation of heat which can be stated as;

Heat lost by hotter body = Heat gained by colder body.

The formula for calculating quantity of heat, q is given as;

q = mcθ

where

m is mass of substance
c is heat capacity of substance
θ is temperature change

Heat losses in a calorimeter will lower the value of enthalpy change, ΔH, for a particular reaction.

Error in the volume of substances used will affect the value of the heat generated, the ΔT observed, the q calculated, and the Δ H calculated as follows:

the heat generated will increase
the ΔT observed will increase
the value of q will increase
the value of ΔH will increase

If the calorimeter used, (Styrofoam cup) is wet when used, the volume of the liquid to be heated will be higher. Therefore, the heat generated, the ΔT observed, the q calculated, and the calculated ΔH will be affected as follows:

the heat generated will decrease
ΔT observed will be lower
the value of q will decrease
the value of ΔH will increase

Learn more about calorimeter at: https://brainly.com/question/1407669