Consider the reaction: 8 H2 S(g)+4 O2(g) ⟶8 H2 O(g)+S8(g) Complete the table. Δ[H2 S] / Δt

Consider the reaction: 8 H2 S(g)+4 O2(g) ⟶8 H2 O(g)+S8(g)...

Consider the reaction: $$ 8 \mathrm{H}_{2} \mathrm{~S}(g)+4 \mathrm{O}_{2}(g) \longrightarrow 8 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{S}_{8}(g) $$ Complete the table. $$ \begin{aligned} &\Delta\left[\mathrm{H}_{2} \mathrm{~S}\right] / \Delta t \quad \Delta\left[\mathbf{0}_{2}\right] / \Delta t \quad \Delta\left[\mathrm{H}_{2} 0\right] / \Delta t \quad \Delta\left[\mathrm{S}_{8}\right] / \Delta t \quad \text { Rate } \\ &-0.080 \mathrm{M} / \mathrm{s} \end{aligned} $$

Consider the reaction:
$$
8 \mathrm{H}_{2} \mathrm{~S}(g)+4 \mathrm{O}_{2}(g) \longrightarrow 8 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{S}_{8}(g)
$$
Complete the table.
$$
\begin{aligned}
&\Delta\left[\mathrm{H}_{2} \mathrm{~S}\right] / \Delta t \quad \Delta\left[\mathbf{0}_{2}\right] / \Delta t \quad \Delta\left[\mathrm{H}_{2} 0\right] / \Delta t \quad \Delta\left[\mathrm{S}_{8}\right] / \Delta t \quad \text { Rate } \\
&-0.080 \mathrm{M} / \mathrm{s}
\end{aligned}
$$

Key Concepts

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction, as determined by the balanced chemical equation. It allows us to predict how changes in the concentration of one substance relate to changes in others, ensuring that the law of conservation of mass is maintained throughout the reaction.

Rate of Reaction

The rate of reaction quantifies how quickly reactants are consumed or products are formed over time, typically expressed in terms of concentration change per unit time (e.g., M/s). Understanding reaction rate is crucial for determining the speed at which a chemical reaction proceeds under given conditions.

Concentration Change (?[ ]/?t)

The notation ?[ ]/?t represents the change in concentration of a reactant or product over a specific time interval. This concept is used to express reaction rates in experimental and theoretical studies, linking the macroscopic measurement of concentration to the temporal progress of a reaction.

Stoichiometric Coefficients and Rate Relationships

Stoichiometric coefficients indicate the proportions in which reactants combine and products form. In the context of reaction rates, these coefficients are used to relate the rates of consumption of reactants to the rates of formation of products; for instance, a negative change in concentration for a reactant is scaled by its coefficient relative to a product’s change in concentration.

Sign Convention in Reaction Rates

In reaction rate measurements, reactants are typically assigned a negative sign because their concentrations decrease over time, while products have positive signs as their concentrations increase. Maintaining proper sign conventions is essential for accurately comparing and calculating the rates of reaction and understanding the overall kinetic behavior of the system.

Transcript

00:01 So in this question we've been given a reaction in which 8 moles of h2s derrick with 4 moles of oxygen to form 8 moles of h2o and s8.

00:14 So for us to answer this question, let's first of all look at the rate expressions in terms of the change and concentration of each of those reactants.

00:22 So we'll be using this equation to determine the rate expressions.

00:26 So what we can see here is to say the rate is equal to negative 1.

00:30 Over 8 multiplied by the change in concentration of h2s divided by delta t.

00:40 This is also equal to negative 1 over 4 multiplied by the change in concentration of oxygen with time.

00:50 And this is also equal to 1 over 8 multiplied by the change in concentration with time.

00:58 And this is equal to the rate of change of the concentration.

01:02 Concentration of s8.

01:06 Now that we have this, this is the information that we're going to be using to fill the table that we've been given.

01:12 So in the table we've been given the rate of change of concentration of h2s, that is delta h2s with time.

01:23 This is equal to negative 0 .08 m per second.

01:29 And we have a negative here because our h2s is a reactant.

01:34 Together with the oxygen but our h2o is a product and our s is a product.

01:41 So these have got a positive because as the reaction progresses, they will be forming increasing their concentration, unlike oxygen and hydrogen sulfide, which will be depleted as the reaction or case, hence a negative rate of change...

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