Methanol can be produced by the following reaction: CO(g)+2 H2( g) →CH3 OH(g) How is the rate of

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Methanol can be produced by the following reaction: CO(g)+2...

Methanol can be produced by the following reaction: $\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})$ How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol? $-\frac{\Delta\left[\mathrm{H}_{2}\right]}{\Delta t}=?$ a. $+\frac{2 \Delta\left[\mathrm{CH}_{3} \mathrm{OH}\right]}{\Delta \mathrm{t}}$ b. $+\frac{1 \Delta\left[\mathrm{CH}_{3} \mathrm{OH}\right]}{2 \Delta \mathrm{t}}$ c. $+\frac{\Delta\left[\mathrm{H}_{4}\right]}{\Delta \mathrm{t}}$ d. None of these

Methanol can be produced by the following reaction:
$\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})$
How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol?
$-\frac{\Delta\left[\mathrm{H}_{2}\right]}{\Delta t}=?$
a. $+\frac{2 \Delta\left[\mathrm{CH}_{3} \mathrm{OH}\right]}{\Delta \mathrm{t}}$
b. $+\frac{1 \Delta\left[\mathrm{CH}_{3} \mathrm{OH}\right]}{2 \Delta \mathrm{t}}$
c. $+\frac{\Delta\left[\mathrm{H}_{4}\right]}{\Delta \mathrm{t}}$
d. None of these

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Key Concepts

Reaction Rate

Reaction rate refers to the change in concentration of reactants or products per unit time. It provides a measure of how quickly a chemical reaction proceeds. The rate can be expressed as a decrease in reactant concentration or an increase in product concentration over time, and it is commonly represented with a negative sign for reactants and a positive sign for products.

Stoichiometry

Stoichiometry deals with the quantitative relationships between reactants and products in a balanced chemical reaction. It provides the mole ratios that determine how much of each substance is involved in the reaction. This concept is critical for linking the rates of formation or consumption of different species in the reaction.

Rate Expression Using Stoichiometry

In stoichiometric reactions, the rate at which reactants are consumed or products are formed is directly related to their coefficients in the balanced equation. This concept allows the conversion of rates from one substance to another by scaling according to the stoichiometric ratios, such as adjusting for a reactant that is consumed in a 2:1 ratio relative to a product.

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