an energy value of 3.313x10^-19 joules is needed to break a chemical bond. what is the wavelength of energy needed to break the bond? (the speed of light = 3.00x10^10 cm/sec; planck's constant = 6.636x10^-34 J . sec
is there a formula i'm missing?
Formula (memorize this)
Energy = frequency * plancks constant.
find the frequency, then (memorize this)
frequency*wavelength= speedlight
The formula you need is the Einstein photoelectric effect equation;
h c/(wavelength) = Energy required
In this case, the equation is applied to radiative chemical dissociation, or "photolysis".
They have given you c (the light speed) and h (Planck's constant). Solve for the wavelength
thanks so much, that one really confused me.
Oh, I'm here to help with confusing stuff! And don't worry, I also get confused by all those equations sometimes. So, let's tackle this together!
Given that the energy required to break the chemical bond is 3.313x10^-19 joules, we can use the Einstein photoelectric effect equation:
wavelength = h * c / Energy
Plugging in the values you provided, we have:
wavelength = (6.636x10^-34 J * sec) * (3.00x10^10 cm/sec) / (3.313x10^-19 J)
Now, let's do some math magic:
wavelength = (6.636 * 3.00) * (10^-34 * 10^10) / (3.313 * 10^-19)
wavelength = (19.908) * (10^-24) / (0.0003313)
wavelength = 60,000 cm
So, the wavelength of energy needed to break the bond is approximately 60,000 centimeters. See, it's not that confusing when you break it down!
You're welcome! I understand that the concept can be confusing, but I'll help you through it step-by-step. Let's break it down:
Given:
Energy (E) = 3.313x10^-19 J
Speed of light (c) = 3.00x10^10 cm/sec
Planck's constant (h) = 6.636x10^-34 J.sec
We can use the equation h c/(wavelength) = Energy to find the wavelength.
Step 1: Rearrange the equation to solve for the wavelength (λ):
wavelength = h c/Energy
Step 2: Substitute the given values into the equation:
wavelength = (6.636x10^-34 J.sec * 3.00x10^10 cm/sec) / (3.313x10^-19 J)
Step 3: Simplify the equation:
wavelength = (1.9908x10^-23 J.cm) / (3.313x10^-19 J)
Step 4: Divide the numerator by the denominator:
wavelength = 6.011x10^-5 cm
Therefore, the wavelength needed to break the chemical bond is approximately 6.011x10^-5 cm.
You're welcome! I understand that the equation may seem confusing at first, but breaking it down step by step can make it easier to comprehend.
First, let's rearrange the equation to solve for wavelength. The equation is:
wavelength = (Planck's constant * speed of light) / energy
Now, plug in the known values:
Planck's constant = 6.636x10^-34 J·s
Speed of light = 3.00x10^10 cm/sec
Energy = 3.313x10^-19 J
Substitute these values into the equation and perform the calculation:
wavelength = (6.636x10^-34 J·s * 3.00x10^10 cm/sec) / (3.313x10^-19 J)
To simplify the units, convert cm/sec to m/sec by multiplying by 100:
wavelength = (6.636x10^-34 J·s * 3.00x10^12 m/sec) / (3.313x10^-19 J)
Perform the multiplication and division:
wavelength ≈ 6.34x10^-7 m
So, the wavelength of the energy needed to break the chemical bond is approximately 6.34x10^-7 meters.
Remember to always double-check your calculations and units to ensure accuracy.