To determine the new rate of the reaction at 30°C, we can use the Arrhenius equation, which relates the rate constant (k) of a reaction to the temperature (T) and the activation energy (Ea). The Arrhenius equation is given by:

k = A * e^(-Ea/RT)

Where:
- k is the rate constant
- A is the pre-exponential factor or frequency factor
- Ea is the activation energy
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin

Given that the rate of the reaction at 10°C is 5, we can assume that the rate constant (k) at 10°C is also 5. We can use this information to find the pre-exponential factor (A) for the reaction.

Now, let's convert the temperatures to Kelvin:
- 10°C = 10 + 273.15 = 283.15 K
- 30°C = 30 + 273.15 = 303.15 K

We can rearrange the Arrhenius equation to solve for the new rate constant (k2) at 30°C:

k2 = k1 * e^((Ea/R) * (1/T1 - 1/T2))

Substituting the known values:
k2 = 5 * e^((Ea/8.314) * (1/283.15 - 1/303.15))

By calculating this expression, we can find the new rate constant (k2) at 30°C.

Question

To determine the new rate of the reaction at 30°C, we can use the Arrhenius equation, which relates the rate constant (k) of a reaction to the temperature (T) and the activation energy (Ea). The Arrhenius equation is given by:

k = A * e^(-Ea/RT)

Where:
- k is the rate constant
- A is the pre-exponential factor or frequency factor
- Ea is the activation energy
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin

Given that the rate of the reaction at 10°C is 5, we can assume that the rate constant (k) at 10°C is also 5. We can use this information to find the pre-exponential factor (A) for the reaction.

Now, let's convert the temperatures to Kelvin:
- 10°C = 10 + 273.15 = 283.15 K
- 30°C = 30 + 273.15 = 303.15 K

We can rearrange the Arrhenius equation to solve for the new rate constant (k2) at 30°C:

k2 = k1 * e^((Ea/R) * (1/T1 - 1/T2))

Substituting the known values:
k2 = 5 * e^((Ea/8.314) * (1/283.15 - 1/303.15))

By calculating this expression, we can find the new rate constant (k2) at 30°C.

Knowee AI · Accepted Answer

To determine the new rate of the reaction at 30°C, we can use the Arrhenius equation, which relates the rate constant (k) of a reaction to the temperature (T) and the activation energy (Ea). The Arrhenius equation is given by:

k = A * e^(-Ea/RT)

Where:
- k is the rate constant
- A is the pre-exponential factor or frequency factor
- Ea is the activation energy
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin

Given that the rate of the reaction at 10°C is 5, we can assume that the rate constant (k) at 10°C is also 5. We can use this information to find the pre-exponential factor (A) for the reaction.

Now, let's convert the temperatures to Kelvin:
- 10°C = 10 + 273.15 = 283.15 K
- 30°C = 30 + 273.15 = 303.15 K

We can rearrange the Arrhenius equation to solve for the new rate constant (k2) at 30°C:

k2 = k1 * e^((Ea/R) * (1/T1 - 1/T2))

Substituting the known values:
k2 = 5 * e^((Ea/8.314) * (1/283.15 - 1/303.15))

By calculating this expression, we can find the new rate constant (k2) at 30°C.

If the rate of a reaction is 5 at 10oC then on increasing the temperature to 30oC,new rate is:

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