Chlorophyll, the green pigment in leaves, has the formula C55H72MgN4O5. If 4.5g of Mg is available to a plant for chlorophyll synthesis, how many grams of carbon will be required to completely use up the magnesium? (enter only your numeric answer, not in scientific notation, and with 1 decimal place)
oops. My solution needs work. I left out a step. It should be this.
4.5 g Mg x (mm C55H72MgN4O5/am Mg) x (55/mm C55H72MgN4O5) x 12 = grams Carbon.
A shorter solution is 4.5 g Mg x (55*am C/am Mg) = grams carbon. Sorry about that.
To determine the number of grams of carbon required to completely use up the magnesium available, we need to calculate the molar ratio between magnesium (Mg) and carbon (C) in the formula of chlorophyll.
First, let's find the molar mass of magnesium (Mg) and carbon (C):
- Molar mass of Mg = 24.3 g/mol
- Molar mass of C = 12.0 g/mol
Next, let's find the ratio between Mg and C in the chlorophyll formula:
- For every 1 Mg atom, there are 55 C atoms, as indicated by the formula C55H72MgN4O5.
Now, let's calculate the number of moles of Mg available by dividing the mass given (4.5 g) by the molar mass of Mg:
Number of moles of Mg = 4.5 g / 24.3 g/mol = 0.185 moles of Mg
Since the ratio between Mg and C is 1:55, we multiply the number of moles of Mg by 55 to find the number of moles of C required:
Number of moles of C = 0.185 moles of Mg * 55 = 10.175 moles of C
Finally, multiply the number of moles of C by the molar mass of C to convert it to grams:
Mass of C = 10.175 moles of C * 12.0 g/mol = 122.1 grams of C
Therefore, the grams of carbon required to completely use up the available magnesium is approximately 122.1 grams (rounded to 1 decimal place).
It takes 55 moles of C to use up each mole of Mg.
So, how many moles of Mg is 4.5g?
mm = molar mass
am = atomic mass
4.5 g Mg x (mm C55H72MgN4O5/am Mg)*55 = g C