Question
the decomposition of hydrogen peroxide in the presence of a catalyst at standard pressure and room temperature is given by the unbalanced chemical equation below.
H_2O_2 (aq) - >H_2O (litre) +O_2(g)
Take the molar gas volume (Vm) as 24,45 dm^3 at room temperature and standard temperature.
how would a catalyst affect the reaction
H_2O_2 (aq) - >H_2O (litre) +O_2(g)
Take the molar gas volume (Vm) as 24,45 dm^3 at room temperature and standard temperature.
how would a catalyst affect the reaction
Answers
GPT-4o mini
A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. In the case of the decomposition of hydrogen peroxide (H₂O₂) into water (H₂O) and oxygen gas (O₂), the presence of a catalyst would primarily affect the reaction in the following ways:
1. **Increased Rate of Reaction**: A catalyst lowers the activation energy required for the reaction to occur, allowing the reaction to proceed more quickly. Therefore, with a catalyst, the decomposition of hydrogen peroxide would happen faster than it would without a catalyst.
2. **No Change in Equilibrium Position**: While a catalyst speeds up the rate at which equilibrium is reached, it does not change the position of the equilibrium itself. This means that the proportions of reactants and products at equilibrium remain the same irrespective of whether a catalyst is present or not.
3. **Lower Activation Energy**: The catalyst provides an alternative reaction pathway with a lower activation energy compared to the uncatalyzed reaction. This makes it easier for the hydrogen peroxide molecules to decompose.
4. **Temperature and Pressure Independence**: Catalysts function under a wide range of temperatures and pressures. Hence, even at standard temperature and room temperature, the catalyst would maintain its effectiveness in speeding up the reaction.
In summary, the use of a catalyst in the decomposition of hydrogen peroxide would result in a faster generation of water and oxygen gas, while keeping the equilibrium concentrations unchanged.
1. **Increased Rate of Reaction**: A catalyst lowers the activation energy required for the reaction to occur, allowing the reaction to proceed more quickly. Therefore, with a catalyst, the decomposition of hydrogen peroxide would happen faster than it would without a catalyst.
2. **No Change in Equilibrium Position**: While a catalyst speeds up the rate at which equilibrium is reached, it does not change the position of the equilibrium itself. This means that the proportions of reactants and products at equilibrium remain the same irrespective of whether a catalyst is present or not.
3. **Lower Activation Energy**: The catalyst provides an alternative reaction pathway with a lower activation energy compared to the uncatalyzed reaction. This makes it easier for the hydrogen peroxide molecules to decompose.
4. **Temperature and Pressure Independence**: Catalysts function under a wide range of temperatures and pressures. Hence, even at standard temperature and room temperature, the catalyst would maintain its effectiveness in speeding up the reaction.
In summary, the use of a catalyst in the decomposition of hydrogen peroxide would result in a faster generation of water and oxygen gas, while keeping the equilibrium concentrations unchanged.