Question

I'm trying to use an self-constructed calorimeter (as shown in picture), which is constructed by two different size test tube and a stopper on the top. I'm using this calorimeter to measure reaction heat as shown below

Mg(s)+2H+ (qq)→Mg₂+ (aq)+H₂( g) ΔH₁
MgO(s)+2H+ (aq)→Mg₂+ (aq)+H₂O(l) ΔH₂
1. Considering the first reaction would produce hydrogen gas, how do I prevent explosion and heat loss at the same time. (I could make the hole bigger on the stopper. But this would create a greater heat loss while doing so.)
2. If I want to speed up the process, should I use concentrated hydrochloric acid without dilution. Is there any safety issue I should think of?

Answer 1

To prevent explosion and heat loss in the self-constructed calorimeter, you can make the hole in the stopper larger and insulate the calorimeter. Concentrated hydrochloric acid can be used to speed up the process, but safety precautions must be taken.

Step-by-step explanation:

To prevent explosion and heat loss while using the self-constructed calorimeter, you can make the hole in the stopper larger to allow the hydrogen gas to escape.

However, this may increase heat loss. To minimize heat loss, you can insulate the calorimeter by adding insulating materials around it. This will help retain the heat produced during the reaction.

If you want to speed up the process, using concentrated hydrochloric acid without dilution can increase the reaction rate.

However, it's important to consider safety issues. Concentrated acids are corrosive and can cause burns and other hazards. Make sure to handle them with care, wear appropriate protective equipment, and work in a well-ventilated area.