Reaction Quotient Calculator
Calculate the reaction quotient (Q) and predict the shift direction relative to Kc.
Calculation Parameters
Adjust the values below.
Calculated Result
Expert Tip
Ensure units are correctly formatted (e.g. Kelvin for gas temperatures and liters for volumes) to get chemically accurate outputs.
How this Calculator Works
This calculator allows you to solve Reaction Quotient problems dynamically. Adjust the input parameters using the sliders or selection menu below:
- Reactant [A] (M) (Range: 0.01 to 5.00, Default: 1.00)
- Reactant [B] (M) (Range: 0.01 to 5.00, Default: 1.00)
- Product [C] (M) (Range: 0.01 to 5.00, Default: 1.20)
- Product [D] (M) (Range: 0.01 to 5.00, Default: 1.20)
- Equilibrium Constant (Kc) (Range: 0.01 to 10.00, Default: 1.00)
The results are computed instantly and updated in the results panel on the right.
Formula & Methodology
If Q < Kc: Shifts Right (Products) | If Q > Kc: Shifts Left (Reactants) | If Q = Kc: Equilibrium
Where:
- Reactant [A]: Parameter value.
- Reactant [B]: Parameter value.
- Product [C]: Parameter value.
- Product [D]: Parameter value.
- Equilibrium Constant: Parameter value.
Step-by-Step Calculation Example
To calculate Reaction Quotient manually, follow these steps:
- Identify the input parameters. For example:
- Reactant [A] (M) = 1.00
- Reactant [B] (M) = 1.00
- Product [C] (M) = 1.20
- Product [D] (M) = 1.20
- Equilibrium Constant (Kc) = 1.00
- Apply the formula:
Q = ([C]^c * [D]^d) / ([A]^a * [B]^b)
If Q < Kc: Shifts Right (Products) | If Q > Kc: Shifts Left (Reactants) | If Q = Kc: Equilibrium - Verify the calculated value which is updated instantly in the results panel on the right.
Frequently Asked Questions
What is the reaction quotient (Q)? ▼
Q is the ratio of product concentrations to reactant concentrations calculated at any non-equilibrium point in time.
What does Q < K indicate? ▼
When Q < K, the reaction shifts to the right (forward direction) toward products to achieve equilibrium.
What does Q > K indicate? ▼
When Q > K, the reaction shifts to the left (reverse direction) toward reactants to achieve equilibrium.