Balance the following equations, and name each reactant and...

Balance the following equations, and name each reactant and product: (a) $\mathrm{SF}_{4}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{SO}_{2}(\mathrm{g})+\mathrm{HF}(\ell)$ (b) $\mathrm{NH}_{3}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{aq}) \rightarrow \mathrm{NO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)$ (c) $\mathrm{BF}_{3}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{HF}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{BO}_{3}(\mathrm{aq})$

Balance the following equations, and name each reactant and product:
(a) $\mathrm{SF}_{4}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{SO}_{2}(\mathrm{g})+\mathrm{HF}(\ell)$
(b) $\mathrm{NH}_{3}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{aq}) \rightarrow \mathrm{NO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $\mathrm{BF}_{3}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{HF}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{BO}_{3}(\mathrm{aq})$

Key Concepts

States of Matter in Chemical Reactions

This pertains to correctly identifying and representing the physical states (solid, liquid, gas, aqueous) of the reactants and products in chemical equations. It provides additional context for the reaction conditions and influences the reaction's behavior.

Chemical Nomenclature

This concept covers the systematic naming of chemical substances according to internationally accepted guidelines. It is crucial for correctly identifying compounds and understanding their properties and behaviors in a reaction.

Identification of Reactants and Products

This key concept involves recognizing and naming the substances present at the beginning (reactants) and the end (products) of the chemical reaction, which is essential for understanding the reaction process and the transformation of chemicals.

Balancing Chemical Equations

This involves adjusting the coefficients of reactants and products to ensure that the number of atoms for each element is equal on both sides of the equation. It is a method that reflects the law of conservation of mass and is fundamental for accurately representing chemical reactions.

Law of Conservation of Mass

This concept states that matter cannot be created or destroyed in a chemical reaction, so the total number of atoms for each element must remain the same on both the reactant and product sides of a balanced equation.

Transcript

00:01 Hello friends, in this video we will learn how to balance chemical equations.

00:05 So we will take few examples.

00:07 So our first example is sf4 reacting with water to give s .o2 plus hf.

00:14 So first let's try to write the names of these compounds.

00:18 So we have sf4, so there is sulfur and there are four atoms of fluorine.

00:24 So it will be sulfur fluoride.

00:31 Then next we already know h2o is water molecule then we have so2 so there are two atoms of oxygen so it will be sulfur dioxide then we have hf which is hydrogen fluoride okay so let's now try to balance this so let's make a note of the different atoms of different elements how many are there on each side so we can write reactant side and product side so we have sulfur, we have fluorine, we have oxygen and we have hydrogen.

01:33 So we have to see how many atoms of these elements are present on both sides.

01:42 So always remember the rule.

01:44 So we have to balance first the metal atoms, then the non -metal atoms, then oxygen atoms and then hydrogen atom.

01:58 Okay, so first let's make a note of how many atoms of each element are there on the two sides.

02:06 So, sulfur is one on both the sides.

02:09 Fluorine is four on the reactant side and one on the product side.

02:14 Oxygen is one on the reactant side and two on the product side.

02:21 And hydrogen is two on the reactant side and one on the product side.

02:26 Right, so let's try to balance these.

02:28 So, sulfur, it's like already balanced.

02:31 Fluorine is 4 here and 1 on the product side.

02:35 So let's try to balance this first...