Thread: Regarding the Law of Conservation of Mass

Hello, everyone. I'm sorry that I'm a noob when it comes to science, but I really need help on this chemistry question.

The original procedure was:
Take a small amount of NaHCO3 in a small beaker and add vinegar to it. Insert a burning splint into the test tube as the reaction happens. What happens? Why?

Okay, so I have that part, but I'm confused on the next part.

Thinking Question:
The Law of Conservation of Mass states that the total mass of the reactants equals the total mass of the products in any chemical reaction. A student tries to verify this law using the above reaction. The student finds out that the law is not getting verified if this reaction is used. Briefly describe what the student would have done to verify the law and why the results did not verify the law directly.

Thanks so much in advance to the person who can answer this question correctly!

Originally Posted by PhDemon

To try and help you out, I suggest you write down the chemical equation for the reaction. What gas is given off? Does this gas support combustion and based on this answer what will it do to a lit splint?

EDIT TO ADD: I see on re-reading you have the answer to the first part...

For the next part did you weight the gas given off in the reaction? If not there is your missing mass right there. To verify the law collect the gas, measure it's volume and from the ideal gas law you can calculate the number of moles and the mass of gas. If the mass of the gas is added to the mass of the other products mass is seen to be conserved.

Thank you!!! I love you!!!!

Originally Posted by PhDemon

Originally Posted by Daklip

Thank you!!!

You're welcome.

Originally Posted by Daklip

I love you!!!!

Sorry, I got a little excited there...I didn't realize how simple the answer was, but I was searching for it for hours!!