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

Average rate = Δ[A]/Δt = (0.8 - 0.4) / 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.

According to Le Chatelier's principle, decreasing the concentration of a reactant will shift the equilibrium to the left to produce more reactants.

Increasing the concentration of a reactant will shift the equilibrium position to the right, favoring the formation of products.

According to Le Chatelier's principle, if the concentration of products increases, the equilibrium will shift to the left.

Decreasing the concentration of products will shift the equilibrium to the right to produce more products, according to Le Chatelier's principle.

According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium to the left, favoring the formation of reactants.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to produce more products.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium to the right to form more products.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to produce more products.

According to Le Chatelier's principle, if the concentration of reactants is increased, the equilibrium will shift to the right to produce more products.

For an exothermic reaction, decreasing the temperature shifts the equilibrium to the right, favoring the formation of products.

For an exothermic reaction, increasing the temperature shifts the equilibrium position to the left, favoring the reactants.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

For an endothermic reaction, increasing temperature shifts the equilibrium to the right, increasing Kc.

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.

The slowest step in a reaction mechanism that determines the overall rate of the reaction is called the rate-determining step.

According to the balanced equation 2H2 + O2 → 2H2O, 2 moles of H2 produce 2 moles of H2O.

If ΔH is negative and ΔS is positive, ΔG will always be negative at all temperatures.

At high temperatures, ΔG will be positive because the positive ΔH and negative ΔS will dominate the equation ΔG = ΔH - TΔS.

2H2 + O2 → 2H2O. 1 mole of water weighs 18 g, so 2 moles produce 36 g. Thus, 18 g of water is produced from 1 mole of O2.

2 moles of H2 and 1 mole of O2 produce 2 moles of H2O. The molar mass of water is 18 g/mol, so 2 moles produce 36 g.

The mole ratio of A to C is 3:4 based on the coefficients in the balanced equation.

For a first-order reaction, if [A] is halved, the rate also halves.

If the rate decreases to one-fourth when concentration is halved, the reaction is second-order.