A light photon with a frequency of at least 0.0906 x 10^16 Hz is required to split apart hydrogen bromide according to the equation:

HBr(g) --> H(g) + Br(g)
Calculate the energy (kJ) required to break apart a mole of hydrogen bromide. Express answer in scientific notation.

Hmm idk the answer

Energy of 1 photon = h*frequency

Energy of 1 mol of photons is that x 6.02E23 in J. Divide by 1000 to convert to kJ.

thank you very much that was great help..

To calculate the energy required to break apart a mole of hydrogen bromide (HBr), we need to use the equation E = hν, where E represents the energy, h is Planck's constant (6.626 x 10^-34 J·s), and ν is the frequency of the light photon.

First, we can convert the given frequency into Hz by multiplying it by 10^16:
Frequency (ν) = 0.0906 x 10^16 Hz

Next, we can substitute the values into the equation:
E = (6.626 x 10^-34 J·s) x (0.0906 x 10^16 Hz)

Now, we can multiply the numerical values together and combine the powers of 10:
E = 6.626 x 0.0906 x 10^-34 x 10^16 J

To simplify the calculation, we can add the exponents of 10:
E = 6.626 x 0.0906 x 10^-34+16 J

Next, we can calculate the product of 6.626 and 0.0906:
E = 0.5991976 x 10^-34+16 J

Now, we can combine the exponents of 10 again:
E = 0.5991976 x 10^-18 J

Finally, we can convert the energy from joules to kilojoules by dividing by 1000:
E = 0.5991976 x 10^-18 J / 1000

Now, we can express the answer in scientific notation by combining the number and exponent of 10:
E = 5.991976 x 10^-21 kJ

Therefore, the energy required to break apart a mole of hydrogen bromide is approximately 5.991976 x 10^-21 kJ.