A light photon with a frequency of at least 0.0906 �~ 1016 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.
See the post above.
To calculate the energy required to break apart a mole of hydrogen bromide (HBr), we can use the equation:
E = hν
where E is the energy, h is the Planck's constant, and ν is the frequency of the light photon.
First, let's convert the given frequency to scientific notation:
0.0906 x 10^16 Hz
Now, we need to find the value of h. Planck's constant, h, is approximately 6.626 x 10^-34 J·s.
Next, we will use the equation to calculate the energy:
E = (6.626 x 10^-34 J·s) × (0.0906 x 10^16 Hz)
Multiplying these values together, we have:
E = 5.998436 x 10^-18 J
Finally, we need to convert Joules to kilojoules. Since 1 kJ is equal to 1000 J, we divide the energy value by 1000:
E = 5.998436 x 10^-18 J ÷ 1000
Simplifying, we get:
E = 5.998436 x 10^-21 kJ
Therefore, the energy required to break apart a mole of hydrogen bromide is 5.998436 x 10^-21 kJ in scientific notation.