Hi can someone help me with this other problem from my homework,
The thermochemical equation is
C6H12O6(s)+ 6O2(g)--> 6CO2(g)+ 6H2O(g)
reaction is -2539.01 kJ/mol
Part B) What is the minimum number of photons with wavelength of 645nm needed to prepare 135 grams of glucose?
Please give me some good information so, I will know how to do it on my own.
1) calculate the energy in a photon in 645 nm (Planck's equation).
2) determine the moles in 135g glucose.
3) determine the energy required: molesglucose*Reactionenergy/mole
4) divide the energy required by the energy in one photon.
Work out the energy associated with each photon of wavelength 645 nm using
E=hf (you will need to convert 645 nm to a frequency first)
Calculate the molecular mass of glucose
Calculate the number of moles of glucose in 135 g
Multiply 2539.01 kJ/mol by the number of moles to get the kJ required.
divide the energy required by the energy of each photon to get the minimum number of photons.
Don't you go back and read your posts? I solved this problem for you the first time you posted. This is a duplicate post and you took the time of THREE volunteers to answer the same one question.
To solve this problem, we need to utilize a concept called the mole-mole ratio and the concept of energy contained in photons.
First, let's determine the mole-mole ratio by examining the balanced chemical equation:
C6H12O6(s) + 6O2(g) --> 6CO2(g) + 6H2O(g)
From the equation, we can see that for every 1 mole of glucose (C6H12O6), 6 moles of carbon dioxide (CO2) are produced.
Now, to calculate the number of moles of glucose present in 135 grams of glucose, we need to use its molar mass.
The molar mass of glucose (C6H12O6) can be calculated by summing the atomic masses of its constituent elements:
Carbon (C): 6 * atomic mass of carbon
Hydrogen (H): 12 * atomic mass of hydrogen
Oxygen (O): 6 * atomic mass of oxygen
Using the periodic table, we find that the atomic masses are approximately:
Carbon (C): 12.01 g/mol
Hydrogen (H): 1.01 g/mol
Oxygen (O): 16.00 g/mol
Now, we can calculate the molar mass of glucose:
Molar mass of glucose = (6 * atomic mass of carbon) + (12 * atomic mass of hydrogen) + (6 * atomic mass of oxygen)
Next, we can calculate the number of moles of glucose:
Number of moles of glucose = Mass of glucose / Molar mass of glucose
Once you have the number of moles of glucose, you can use this information to determine the number of moles of carbon dioxide produced using the mole-mole ratio from the balanced equation.
Now, let's move on to the second part of the question, which involves determining the number of photons with a wavelength of 645 nm needed.
The energy contained in a single photon can be determined using the equation:
Energy = Planck's constant (h) * speed of light (c) / wavelength
Planck's constant (h) is approximately 6.626 x 10^-34 J·s, and the speed of light (c) is approximately 3.00 x 10^8 m/s.
Now, you can calculate the energy of a single photon with a wavelength of 645 nm using the equation:
Energy of a single photon = (Planck's constant * speed of light) / wavelength
Finally, to find the minimum number of photons required to prepare 135 grams of glucose, you need to divide the energy required to produce 135 grams of glucose by the energy of a single photon.
I hope this explanation helps you understand how to approach the problem. If you have any further questions, feel free to ask!