For part 1 (which is below), we will make the assumption that the measured delta

Question

For part 1 (which is below), we will make the assumption that the measured deltaH is H . Is this a reasonable assumption? Briefly explain.

Part 1. Determination of deltaH is ( H )

Obtain a calorimeter and replace the metal cup inside with a 100-ml beaker. Add 50.0 mL of water to the calorimeter and record the initial temperature of the water. Weigh 2-3 g of urea (record actual value) and rapidly add to the water with good mixing. You want to make sure that all of the urea dissolves relatively quickly in order to get the best temperature measurement. Read and record the final temperature of the solution immediately after the urea has completely dissolved.

Explanation / Answer

As I can understand in your exercise the measured Delta H will be incorrect, Why? Because Delta H has to be measured in an closed system, also, there is not only temperature involve in that change, there is also change in volume, work done by the system, and on the system itself, in the moment you are mixing your solution you are adding energy that was not initially standarized. Thats my apreciation without any other data

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