Calorimetry question (unaccounted heat loss)

In summary, the conversation discusses the impact of unaccounted for heat loss on the measurement of the enthalpy of neutralization for an acid-base reaction. The formula for calculating enthalpy of neutralization is mentioned, and the conversation delves into the possibility of heat loss being so fast that it is not observed by the calorimeter. The use of different materials for the calorimeter is also discussed, with the conclusion that glass may result in a greater temperature change due to its better heat conductivity. The conversation ends with a comment on the nature of these types of questions and their purpose.
  • #1
FLgirl
21
0
1. An acid-base neutralization reaction is exothermic. For the measurement of the enthalpy of neutralization, for the reaction, heat is inevitably lost to the calorimeter (beaker or styrofoam cup). How will this unaccounted for heat loss affect the reported value for the enthalpy of neautralization for the reaction?



2. enthalpy (heat) of neutralization = heat released by neutralization reaction / moles of acid or base that react



3. The Attempt at a Solution ..I'm stumped, I need someone smarter than me to explain this to me.
 
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  • #2
Imagine the heat is lost so fast you don't observe a temperature change inside the calorimeter. What would be the determined enthalpy of neutralization?
 
  • #3
Considering you didn't answer my question... how does that explain anything?
 
  • #4
It does. If you don't see how, please answer and I will try to guide you to the moment when you will understand.
 
  • #5
Think about your tools... the thermometer itself has to react in order to measure the temperature change. If it's measurement is off (as all measurements are), then how will that affect your analysis of what's happening?

If you've actually lost 10 units, but your measurement is showing that you lost 8 units, how will that affect your calculations?
 
  • #6
ps.:
1. Will the recorded temperature change for an exothermic reaction performed in a glass calorimeter be greater or less than that in a styrofoam coffee cup calorimeter? Assume glass to be a better conductor of heat than styrofoam.
If glass is a better conductor, then heat will move through it faster, right? If more heat leaves rather than being measured by the thermometer, then... ?

By the way, I hate these questions. They're dumb, because this is stuff that you'll come to realize on your own. This crap is just teachers trying to come up with something to trip up some students to prevent everyone from getting good grades. It's dumb.
 

1. What is calorimetry and how does it work?

Calorimetry is a scientific technique used to measure the amount of heat energy released or absorbed during a physical or chemical process. It works by using a calorimeter, which is an insulated container that contains a known quantity of water. The heat released or absorbed by a substance is transferred to the water, causing a change in its temperature. By measuring this change in temperature, the amount of heat released or absorbed can be calculated.

2. How do you calculate the heat lost in a calorimetry experiment?

The heat lost in a calorimetry experiment is calculated by using the formula Q = m x c x ΔT, where Q is the heat lost, m is the mass of the substance, c is the specific heat capacity of the substance, and ΔT is the change in temperature. This formula takes into account the mass and specific heat capacity of the substance, as well as the change in temperature, to accurately calculate the heat lost.

3. What factors can contribute to unaccounted heat loss in a calorimetry experiment?

Unaccounted heat loss in a calorimetry experiment can be caused by a variety of factors such as improper insulation of the calorimeter, heat loss due to evaporation of the substance, heat loss through the container holding the substance, and heat loss due to the surrounding environment. These factors can affect the accuracy of the results obtained from the experiment and should be taken into consideration when conducting calorimetry experiments.

4. How can unaccounted heat loss be minimized in a calorimetry experiment?

To minimize unaccounted heat loss in a calorimetry experiment, it is important to properly insulate the calorimeter to prevent heat from escaping. This can be done by using materials such as Styrofoam or double-walled containers. It is also important to minimize the time the substance is exposed to the surrounding environment and to use a lid on the calorimeter to reduce heat loss through evaporation. Additionally, conducting the experiment in a controlled environment with minimal temperature fluctuations can also help minimize unaccounted heat loss.

5. How does unaccounted heat loss affect the results of a calorimetry experiment?

Unaccounted heat loss can significantly affect the accuracy of the results obtained from a calorimetry experiment. This is because heat loss is not being taken into account and therefore, the calculated heat lost will be lower than the actual value. This can result in an underestimation of the heat released or absorbed by the substance, leading to inaccurate conclusions. It is important to minimize unaccounted heat loss in order to obtain reliable and accurate results from calorimetry experiments.

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