Express the rate of this reaction in terms of the change in concentration of each of the reactants and products: $$ 2 \mathrm{D}(g)+3 \mathrm{E}(g)+\mathrm{F}(g) \longrightarrow 2 \mathrm{G}(g)+\mathrm{H}(g) $$ When [D] is decreasing at \(0.1 \mathrm{~mol} / \mathrm{L} \cdot \mathrm{s}\), how fast is [H] increasing?

Understanding reaction kinetics is crucial in determining the speed at which a chemical reaction occurs. Reaction kinetics studies the factors that affect the rate of a chemical reaction and provides insight into the reaction mechanism.

The rate of a reaction can be expressed as the change in concentration of reactants or products per unit time. It is commonly measured in terms of molarity per second (mol/L·s).

Factors influencing reaction rates include temperature, concentration, surface area, and the presence of catalysts. Higher temperatures and concentrations typically increase reaction rates, as they lead to more frequent and energetic collisions between reactant molecules.

For the given reaction (2D(g) + 3E(g) + F(g) → 2G(g) + H(g)), the rate of the reaction can be analyzed by looking at how the concentrations of 'D', 'E', and 'F' decrease, and how the concentrations of 'G' and 'H' increase over time.

Stoichiometric coefficients are the numbers placed in front of the molecules in a chemical equation. These coefficients indicate the relative amounts of each substance involved in the reaction and are essential for balancing chemical equations.

In the reaction 2D(g) + 3E(g) + F(g) → 2G(g) + H(g), the coefficients 2, 3, 1, 2, and 1 represent the mole ratios of D, E, F, G, and H, respectively. These ratios are vital in expressing the rate of reaction.

When expressing the reaction rate, we use the stoichiometric coefficients to relate the rate of change in concentration of one species to another. For example, if D is consumed at a rate of 0.1 mol/L·s, we can derive the rate at which H is formed using its stoichiometric ratio relative to D. Since H is formed at one-half the rate that D is consumed, the rate of formation of H would be 0.05 mol/L·s.

Concentration change is a key aspect of reaction kinetics. It refers to how the molarity of reactants and products changes over time.

During the reaction, as reactants are converted to products, the concentration of reactants decreases and the concentration of products increases. This change can be measured to determine the reaction rate.

For the reaction 2D(g) + 3E(g) + F(g) → 2G(g) + H(g), if we know that the concentration of D decreases by 0.1 mol/L·s, we can use the stoichiometric coefficients to find how the concentrations of E, F, G, and H change. By using the relationships from the balanced chemical equation, we can affirm that:

• -d[D]/dt = 0.1 mol/L·s
• -d[E]/dt = (3/2) * 0.1 mol/L·s = 0.15 mol/L·s
• -d[F]/dt is at the same rate as it appears with a coefficient of 1
• d[G]/dt = (1/2) * 0.1 mol/L·s = 0.05 mol/L·s
• d[H]/dt = 0.05 mol/L·s

This allows us to see the interrelationship of concentration changes among reactants and products.