Question

What is the mean rate of reaction 3.4g of copper sulphate was produced in 3 days?

please help me ​

Answer 1

The mean rate of reaction for producing 3.4g of copper sulphate in 3 days is 0.00001312 g/s, calculated by dividing the mass of copper sulphate by the total time in seconds.

Step-by-step explanation:

To calculate the mean rate of reaction for the production of copper sulphate, we need to divide the total amount of copper sulphate produced by the time taken for the reaction. Given that 3.4g of copper sulphate was produced in 3 days, we first need to convert days into seconds because the rate of reaction is usually expressed in units of concentration over time.

There are 24 hours in a day, 60 minutes in an hour, and 60 seconds in a minute. Therefore, 3 days is equal to 3×24×60×60 = 259,200 seconds.

Now calculating the mean rate:

Total mass of Copper Sulphate (g) / Total time (s)
= 3.4 g / 259,200 s
= 0.00001312 g/s }

This is the mean rate of reaction for copper sulphate production in this scenario.

Answer 2

8.1×10^-8 mols-1

Step-by-step explanation:

Now we have the mass of copper sulphate produced after three days. Recall that the rate of reaction is given as;

Rate= change in the concentration of product/time

At the beginning of the reaction, there was 0 moles of copper sulphate

After 72 hours or 259200 seconds, there was 3.4g/160gmol-1 = 0.021 moles of copper sulphate.

Note that 160gmol-1 is the molar mass of copper sulphate.

Hence;

Rate of reaction= 0.021 moles /259200 seconds

Hence, the rate of reaction is 8.1×10^-8 mols-1

Rate of reaction= 8.1×10^-8 mols-1