For a first-order reaction, the half-life is independent of the initial concentration. Therefore, it remains 10 minutes.

For a first-order reaction, the half-life is given by the expression t1/2 = 0.693/k.

For a first-order reaction, the half-life is independent of the initial concentration.

The rate of disappearance of A is equal to the rate of formation of B, multiplied by the stoichiometric coefficients. Here, it is 1.0 mol/L/s.

If doubling the concentration of A doubles the rate, the reaction is first order with respect to A.

For a first-order reaction, the rate of reaction is directly proportional to the concentration of the reactant, given by Rate = k[A].

In a zero-order reaction, the rate is constant and does not depend on the concentration of reactants.

In a zero-order reaction, the rate is constant and does not depend on the concentration of the reactants.

According to the Arrhenius equation, an increase in activation energy results in a decrease in the rate constant k.

Using the Arrhenius equation, a rule of thumb states that for every 10°C increase in temperature, the rate doubles if Ea is around 40 kJ/mol.

In a first-order reaction, the half-life is independent of the concentration of the reactant, so it remains the same.

Average rate = (change in concentration) / (time) = (0.5 - 0.1) / 20 = 0.02 M/min.

For the reaction A → B, the rate of disappearance of A is equal to the rate of formation of B, hence it is 0.1 mol/L·s. However, if stoichiometry is considered as 1:1, the rate of disappearance of A is also 0.1 mol/L·s.

For the reaction A → B, the rate of disappearance of A is equal to the rate of formation of B, thus it is 1.0 mol/L·s.

If the rate doubles when the concentration of A is doubled, the reaction is first order with respect to A.

The slowest step in a reaction mechanism is called the rate-determining step, as it controls the overall reaction rate.

The slowest step in a reaction mechanism is known as the rate-determining step.

In a zero-order reaction, the rate is constant and does not depend on the concentration of reactants.

For a zero-order reaction, time = (initial concentration - final concentration) / k = (2 - 0) / 5 = 0.4 s.

In a zero-order reaction, the rate of reaction is independent of the concentration of reactants.

The Arrhenius equation relates the rate constant to temperature and activation energy.

The half-life of a first-order reaction is given by t1/2 = 0.693/k, which depends only on the rate constant.

The rate law for a reaction is determined experimentally and is dependent on the mechanism of the reaction.

The rate law for a reaction depends on the mechanism of the reaction.

The overall order of the reaction is the sum of the powers of the concentration terms, which is 1 + 2 = 3.

This is an example of Van 't Hoff rule, which states that the rate of reaction doubles for every 10°C increase in temperature.

The rate of reaction is expressed in terms of concentration change per unit time, hence the unit is mol/L·s.

This relationship is known as the rate law of the reaction.

Increasing the concentration of a reactant in a first-order reaction increases the rate of the reaction.

A catalyst does not affect the position of equilibrium; it only speeds up the rate at which equilibrium is reached.