If 2.00 g of element G reacts with 5.00 g of element M to produce 7.00 g of a compound with the formula G3M2, what is the atomic mass of G if the atomic mass of M is 135.0 amu?
Answer is 36 amu but why
3G +2M ==> G3M2
mols M = 5.00/135 = approx 0.037
mols G = 0.037 x (3 mols G/2 mols M) = approx 0.0555
Then mols = g/atomic mass. You know mols G and grams G, solve for atomic mass G. I'll bet you get 36.
this man is a savage ^
To find the atomic mass of element G, we need to use the given information about the masses and the formula of the compound.
1. Start by calculating the number of moles of element M:
Moles of M = Mass of M / Atomic mass of M
Moles of M = 5.00 g / 135.0 g/mol = 0.037 mol
2. We can determine the molar ratio between G and M from the formula G3M2. Here, we see that there are three atoms of G for every two atoms of M.
3. Using the molar ratio, we can calculate the number of moles of G by multiplying the moles of M by the ratio:
Moles of G = Moles of M * (3 / 2)
Moles of G = 0.037 mol * (3 / 2) = 0.0555 mol
4. Now, we can calculate the molar mass of element G by dividing the mass of G by the number of moles of G:
Atomic mass of G = Mass of G / Moles of G
Atomic mass of G = 2.00 g / 0.0555 mol = 36.0 g/mol (rounded to two decimal places)
Therefore, the atomic mass of element G is 36 amu.