Sorry to post this again, not sure if it was seen.

If someone has the time to help with the following question it would be really helpful.

Posted by Nancy on Monday, September 22, 2014 at 9:55am.

The problem is
209/83bi+64/28NI=272/111Rg+1/0n
How to calculate the energy change in J/mol reactants?

AMU amounts:
Bi=208.980384
Ni= 63.927969
Rg=272.1535

What I have done is
1. subtract products from reactants.
2. multiply the result by 1.66054x10^-27kg
3. multiply that by 8.98x10^16 (which is c^2 in e=mc^2
4. multiply that result by 6.022x10^23

The answer is 1.03x10^11. But I am not getting that.
can someone explain how to do this problem? I keep getting the following answer which by the book is wrong:

1. difference between reactant and products=.253807 amu
2. .253807 x 1.66054x10^-27=4.2145x10-28
3. 4.2145x10-28x8.98x10^16=3.784x10-11
4. 3.784x10-11 x6.022x10^23=2.279x10^13

The book has 1.03x10^11. Why??

To calculate the energy change in J/mol reactants, you need to use the equation E = mc^2, where E is the energy change, m is the mass difference, and c is the speed of light.

Let's go step by step through the calculations to determine where the discrepancy lies.

1. Find the mass difference between reactants and products:
The mass difference is calculated by subtracting the sum of the product masses from the sum of the reactant masses.
(209/83 Bi + 64/28 Ni) - (272/111 Rg + 1/0 n) = 0.253807 amu

Your calculation is correct.
Difference = 0.253807 amu

2. Convert the mass difference to kg:
Multiply the mass difference by the conversion factor 1.66054x10^-27 kg/amu.
0.253807 amu x 1.66054x10^-27 kg/amu = 4.2145x10^-28 kg

Your calculation is correct.
Mass difference = 4.2145x10^-28 kg

3. Calculate the energy change using E = mc^2:
Multiply the mass difference by the square of the speed of light c, which is approximately 8.98x10^16 m^2/s^2.
E = 4.2145x10^-28 kg x (8.98x10^16 m^2/s^2) = 3.784x10^-11 J

Your calculation is correct.
Energy change = 3.784x10^-11 J

4. Convert the energy change to J/mol:
Multiply the energy change by Avogadro's number, 6.022x10^23 mol^-1.
3.784x10^-11 J x (6.022x10^23 mol^-1) = 2.279x10^13 J/mol

Your calculation is correct, but you made a mistake in the final step.
Energy change = 2.279x10^13 J/mol

So, the correct answer is indeed 2.279x10^13 J/mol, not 1.03x10^11 J/mol as stated in the book. It seems there might be an error in the book's answer.