the hydrolysis of sucrose is a part of the digestive process. to investigate how strongly the rate depends on our body temperature, calculate the rate constant for they hydrolysis of sucrose at 35C given that k=1.0 mL/(mol*s) at 37C and that the Ea=108 kJ/mol

Question

the hydrolysis of sucrose is a part of the digestive process. to investigate how strongly the rate depends on our body temperature, calculate the rate constant for they hydrolysis of sucrose at 35C given that k=1.0 mL/(mol*s) at 37C and that the Ea=108 kJ/mol

Answer 1

Can't you use the Arrhenius equation, just plug in the numbers and turn the crank.

Answer 2

Given that Ea for the hydrolysis of sucrose is 108 ×10³ Kj /Mol, compar the rat of constant of this reaction at 37⁰C (T) with the rate constant of the same reaction at 27⁰C (T)

Answer 3

To calculate the rate constant for the hydrolysis of sucrose at 35°C, we can use the Arrhenius equation. The Arrhenius equation is given as:

k = Ae^(-Ea/RT)

Where:
k is the rate constant
A is the pre-exponential factor
Ea is the activation energy (given as 108 kJ/mol)
R is the ideal gas constant (8.314 J/(mol·K))
T is the temperature in Kelvin (35°C + 273.15 = 308.15 K)

First, let's calculate the pre-exponential factor (A) using the given rate constant (k) at 37°C:

k = 1.0 mL/(mol·s)

Since the units of the rate constant need to be in the same units as the activation energy (kJ/mol), we need to convert mL to L and seconds to seconds per hour:

1 mL = 0.001 L
1 s = 1/3600 h

So, the rate constant (k) at 37°C is:

k = 1.0 mL/(mol·s) * 0.001 L/mL * (1/3600) h/s = 2.78 x 10^-7 L/(mol·h)

Next, we can substitute the known values into the Arrhenius equation and solve for the rate constant (k) at 35°C:

k = Ae^(-Ea/RT)

k(35) = A * e^(-108,000 J/mol / (8.314 J/(mol·K) * 308.15 K))

To convert the activation energy from J/mol to kJ/mol, divide by 1000:

k(35) = A * e^(-108 kJ/mol / (8.314 J/(mol·K) * 308.15 K))

To get the value of the rate constant (k) at 35°C, we need to know the pre-exponential factor (A). If the value of A is not given, it will be difficult to determine the exact rate constant at 35°C without additional information. However, you can still calculate the ratio of rate constants at different temperatures using the Arrhenius equation if you have the value of A or any other ratio of rate constants at different temperatures.