## What is the value of rate constant?

The value of the rate constant is temperature dependent. A large value of the rate constant means that the reaction is relatively fast, while a small value of the rate constant means that the reaction is relatively slow.

## How do you find the value of the rate constant?

To find the rate constant:

- Determine how many atoms are involved in the elementary step of the reaction.
- Find out the order of reaction for each atom involved in the reaction.
- Raise the initial concentration of each reactant to its order of reaction, then multiply them all together.

**What is the value of R in rate law?**

The value of the gas constant, R, is 8.31 J K-1 mol-1.

### Is rate and k the same?

A rate law shows how the rate of a chemical reaction depends on reactant concentration. For a reaction such as aA → products, the rate law generally has the form rate = k[A]ⁿ, where k is a proportionality constant called the rate constant and n is the order of the reaction with respect to A.

### What is K in chemical reaction?

The equilibrium constant of a chemical reaction (usually denoted by the symbol K) provides insight into the relationship between the products and reactants when a chemical reaction reaches equilibrium.

**Does the value of rate constant change?**

The value of rate constant for the same reaction changes with temperature. 4. The value of rate constant for a reaction does’t depend upon the concentration of the reactants.

## What is K in first order reaction?

‘k’ is the rate constant of the first-order reaction, whose units are s-1. ‘[A]’ denotes the concentration of the first-order reactant ‘A’. d[A]/dt denotes the change in the concentration of the first-order reactant ‘A’ in the time interval ‘dt’.

## What is the value of R in Arrhenius equation?

8.314 J/mol-K

The value of the slope (m) is equal to -Ea/R where R is a constant equal to 8.314 J/mol-K. The activation energy can also be found algebraically by substituting two rate constants (k1, k2) and the two corresponding reaction temperatures (T1, T2) into the Arrhenius Equation (2).