Interpret these chemical reactions in terms of the number of...

Interpret these chemical reactions in terms of the number of moles of each reactant and product: (a) $\mathrm{MgBr}_2+2 \mathrm{AgNO}_3 \longrightarrow \mathrm{Mg}\left(\mathrm{NO}_3\right)_2+2 \mathrm{AgBr}$ (b) $\mathrm{N}_2+3 \mathrm{H}_2 \longrightarrow 2 \mathrm{NH}_3$ (c) $2 \mathrm{C}_3 \mathrm{H}_7 \mathrm{OH}+9 \mathrm{O}_2 \longrightarrow 6 \mathrm{CO}_2+8 \mathrm{H}_2 \mathrm{O}$

Interpret these chemical reactions in terms of the number of moles of each reactant and product:
(a) $\mathrm{MgBr}_2+2 \mathrm{AgNO}_3 \longrightarrow \mathrm{Mg}\left(\mathrm{NO}_3\right)_2+2 \mathrm{AgBr}$
(b) $\mathrm{N}_2+3 \mathrm{H}_2 \longrightarrow 2 \mathrm{NH}_3$
(c) $2 \mathrm{C}_3 \mathrm{H}_7 \mathrm{OH}+9 \mathrm{O}_2 \longrightarrow 6 \mathrm{CO}_2+8 \mathrm{H}_2 \mathrm{O}$

Key Concepts

Mole Concept

The mole concept is a fundamental idea in chemistry that defines a mole as a specific number (Avogadro’s number) of particles, whether atoms, molecules, or ions. It allows chemists to count entities in a chemical reaction by using the mass of substances and convert between the mass of a substance and the number of its constituent particles.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It uses the mole ratios provided by the coefficients in the equation to quantify relationships between substances, ensuring that the amounts of reactants and products comply with the reaction’s conditions.

Mole Ratios

Mole ratios refer to the proportional relationship between reactants and products as indicated by the coefficients in a balanced chemical equation. These ratios are essential for determining how many moles of one substance are required or produced when a specific number of moles of another substance reacts or is formed.

Balanced Chemical Equations

A balanced chemical equation accurately represents a chemical reaction by ensuring that the number of atoms for each element is the same on both the reactant and product sides. This balance not only signifies the conservation of mass but also provides the quantitative basis for stoichiometric calculations in the reaction.

Conservation of Mass

The law of conservation of mass states that matter is neither created nor destroyed during a chemical reaction. In the context of balanced chemical equations, this principle guarantees that the total mass of the reactants equals the total mass of the products, which underpins all stoichiometric interpretations and calculations in chemistry.

Transcript

00:01 All right, so for this question, we're given four unbalanced chemical reactions.

00:04 So i'm going to start by balancing them.

00:07 All right, there's one magnesium on either side, one copper on other side, and two quorines on either sides.

00:15 This one's already balanced.

00:16 So another part of this question is to assume that the first reactant, we have 25 grams of it.

00:21 We want to know how many moles of the second reactant do we need to react this exactly? so each one will be, we're assuming that each one will be completely consumed in this reaction.

00:35 So we have 25 grams of the magnesium.

00:50 There's 24, 25 grams per mole of magnesium, which is equal to about one mole of magnesium.

01:03 Now given that the ratio of moles of magnesium to the cucl2, is one to one.

01:13 We can also say that there's about one mole of co, cl2.

01:23 Okay, for b, right, the chlorines aren't equal.

01:31 There's two on the reactant side and only one on the product side, so i'm going to double this product.

01:37 So now, of course, the silvers aren't equal, so i'm going to also double this reactant.

01:41 So now there's two silvers on either side, six oxygens on both sides.

01:48 Two nitrogen on both sides, one nickel on either side, and two chlorines on the other side.

01:57 So this is now balanced...

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