A 1.268 g sample of a metal carbonate, MCO₃, was treated 100.00 mL of 0.1083 M H₂SO₄, yielding CO₂ gas and an aqueous solution of the metal sulfate. The solution was boiled to remove all of the dissolved CO₂ and then was titrated with 0.1241 M NaOH. A 71.02 mL volume of the NaOH solution was required to neutralize the excess H₂SO₄.a) Write the balanced chemical equation for this reaction.
b) What is the identity of the metal?
c) How many grams of CO₂ gas were produced?

MCO3 is BaCO3

The mass of CO2 produced is 0.28g of CO2

Explanation:

The first step in solving the question is to put down the balanced reaction equations as shown in the image attached. Secondly, we obtain the relative number of moles acid and base as mentioned in the question. The balanced neutralization reaction equation is used to obtain the number of moles of excess acid involved in the neutralization reaction.

This is then subtracted from the total number of moles acid to give the number of moles of acid that reacted with MCO3. From here, the molar mass of MCO3 and identity of M can be found. Hence the mass of CO2 produced is calculated as shown.

The reactivity and binding capabilities of carbon are crucial to life due to the different reactions that happen in the environment and in life. Carbon can be found not only in living organisms but also in the atmosphere. Since living organisms need carbon but they are unable to make it for themselves the carbon cycle comes into play. First carbon is found as CO2 in the atmosphere one of the ways that CO2 can get into the atmosphere from humans breathing, producers such as plants use it to make glucose (C6H12O6). The carbon dioxide produced by living things is produced through cellular respiration a process in which cells from living organisms burn glucose to generate energy and as a byproduct, carbon dioxide is released.