Complete and balance the equation for each of the following...

Complete and balance the equation for each of the following reactions: a. $\mathrm{KHCO}_{3}(s)+\operatorname{HBr}(a q) \longrightarrow$ b. $\mathrm{Ca}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow$ c. $\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(s) \longrightarrow$ d. $\mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow$

Complete and balance the equation for each of the following reactions:
a. $\mathrm{KHCO}_{3}(s)+\operatorname{HBr}(a q) \longrightarrow$
b. $\mathrm{Ca}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow$
c. $\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(s) \longrightarrow$
d. $\mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow$

Key Concepts

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the same number of atoms of each element exists on both sides of the equation. This practice is vital because it reflects the law of conservation of mass, meaning that matter is neither created nor destroyed in a chemical reaction.

Stoichiometry

Stoichiometry provides the quantitative relationship between reactants and products in a chemical reaction. It is used to calculate the precise amounts of substances involved, ensuring that the reaction is balanced and that coefficients are correctly assigned according to the mole ratios dictated by the reaction.

Acid-Base Neutralization Reactions

Acid-base neutralization reactions occur when an acid reacts with a base to produce a salt and water. This reaction type is foundational in chemistry, demonstrating the neutralization process where hydrogen ions from the acid and hydroxide ions from the base combine to form water. In many cases, side reactions such as the decomposition of unstable intermediate acids (e.g., carbonic acid) also play a role.

Single Displacement Reactions

Single displacement reactions involve one element in its elemental form displacing another element from a compound. This type of reaction is common when a more reactive metal replaces a less reactive hydrogen in an acid, leading to the formation of a salt and the release of hydrogen gas.

Decomposition Reactions in Acid-Carbonate Interactions

In reactions where carbonates or bicarbonates react with acids, an unstable intermediate such as carbonic acid is often formed. This intermediate frequently decomposes into water and carbon dioxide, impacting the overall balanced chemical equation by introducing gaseous products that need to be accounted for.

Transcript

0:00 Hello.

00:02 In this question we have been given some chemical equations which we have to we have been only given the reactants and we have to write the products and then apart from that we have to balance it as well.

00:13 Okay so let's go to the first one so in the first one kh co3 potassium hydrogen carbonate reacts with hydrogen bromide it gives potassium bromide plus co2 plus h2.

00:39 Okay, so we need to balance it.

00:42 So let's check potassium is already balanced.

00:45 Hydrogen is already balanced.

00:48 Carbon is already balanced and oxygen is also already balanced.

00:52 Okay, so this reaction is already balanced.

00:55 Then we go to the second one, calcium reacting with h2 -s -o -4.

01:01 So it gives you calcium sulfate, which is c -a -s -4 plus h -2.

01:09 Okay, so in this case, hydrogen is already balanced.

01:12 Calcium is already balanced and sulfur and oxygen are also balanced so this is already a balanced equation then next one we go to next one so next is h2 so 4 reacts with calcium hydroxide so that gives you calcium sulfate which is c a so 4 plus h2 that is water so this is the example of a neutralization reaction wherein an acid and a basa reacting okay let's check whether it is balanced or not.

01:53 So calcium is balanced.

01:54 Hydrogen is not yet balanced...

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