When NaHCO3 is heated above 270^∘ C, it decomposes to Na2 CO3(s), H2 O(g), and CO2(g). a. Write

step 1 The question here says that when we have N -H -C -O -3 and we heat it, it decomposes to N -A -2

When NaHCO3 is heated above 270^∘ C, it decomposes to Na2...

When $\mathrm{NaHCO}_{3}$ is heated above $270^{\circ} \mathrm{C},$ it decomposes to $\mathrm{Na}_{2} \mathrm{CO}_{3}(s), \mathrm{H}_{2} \mathrm{O}(g),$ and $\mathrm{CO}_{2}(g)$. a. Write a balanced chemical equation for the decomposition reaction. b. Calculate the mass of $\mathrm{CO}_{2}$ produced from the decomposition of $25.0 \mathrm{g}$ of $\mathrm{NaHCO}_{3}$.

When $\mathrm{NaHCO}_{3}$ is heated above $270^{\circ} \mathrm{C},$ it decomposes to $\mathrm{Na}_{2} \mathrm{CO}_{3}(s), \mathrm{H}_{2} \mathrm{O}(g),$ and $\mathrm{CO}_{2}(g)$.
a. Write a balanced chemical equation for the decomposition reaction.
b. Calculate the mass of $\mathrm{CO}_{2}$ produced from the decomposition of $25.0 \mathrm{g}$ of $\mathrm{NaHCO}_{3}$.

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Key Concepts

Decomposition Reaction

A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more simpler substances. This concept is important in chemistry because it illustrates how compounds can change into different substances under the right conditions, often with the help of energy such as heat.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both sides of the reaction. This is based on the law of conservation of mass, which mandates that atoms are neither created nor destroyed in a chemical reaction.

Stoichiometry

Stoichiometry involves calculating the relationships between reactants and products in a chemical reaction. It uses the coefficients from the balanced chemical equation to determine the proportions and amounts of substances consumed and produced during the reaction.

Molar Mass and Conversions

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole. This concept is essential for converting between the mass of a substance and the number of moles, thereby allowing quantitative calculations in chemical reactions.

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