A sample of 0.30 moles of a metal M reacts completely with excess fluorine to form 18.69 grams of MF2.
How many moles of F are in the sample of MF2 that forms?
M + F2 ---> MF2
How many grams of M are in this sample of MF2 ?
M + F2 ==> MF2
0.3mole M means 0.3 mole F2. How many grams is that? moles F2 x molar mass F2 = g fluorine.
18.69 = g MF2
- grams fluorine
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7.+ grams must be M.
Then moles = g/molar mass and solve for molar mass.
thank you :)
To determine the number of moles of F in the sample of MF2, we first need to find the molar mass of MF2.
Let's assume the molar mass of M is "x".
The molar mass of MF2 can be calculated by adding the molar mass of M (x) to the molar mass of F (which is 19.00 g/mol, as fluorine is a diatomic molecule).
So, the molar mass of MF2 is x + 2(19.00) = x + 38.00 g/mol.
We are given that 0.30 moles of M reacts to form 18.69 grams of MF2.
To find the moles of F in MF2, we can use the mole ratio between M and F in the balanced chemical equation (1:2), which means that for every mole of M, there are 2 moles of F.
Since the molar ratio of M to F in MF2 is 1:2, the number of moles of F in the sample is twice the number of moles of M.
Therefore, the number of moles of F in the sample of MF2 is 2 * 0.30 = 0.60 moles.
To find the grams of M in the sample of MF2, we need to calculate the mass of 0.30 moles of M.
Using the molar mass of M (x), the mass of 0.30 moles of M is 0.30 * x grams.
However, the molar mass of M is unknown, so we cannot find the exact mass of M in the sample without further information.
To find the number of moles of F in the sample of MF2, we need to use the balanced chemical equation and the stoichiometry information.
According to the balanced chemical equation:
1 mole of M reacts with 2 moles of F2 to form 1 mole of MF2.
Given that 0.30 moles of M reacts to form 18.69 grams of MF2, we can use the given information to calculate the number of moles of F.
Step 1: Determine the molar mass of MF2.
From the periodic table,
The molar mass of M = x grams/mol (not given)
The molar mass of F = 19.00 grams/mol.
The molar mass of MF2 = (Molar mass of M) + 2*(Molar mass of F)
= (Molar mass of M) + 2 * 19.00 grams/mol.
However, since the molar mass of M is not given, we cannot directly calculate the exact mass of M in MF2.
Now, let's move on to finding the number of grams of M in MF2.
To determine the number of grams of M in MF2, we can subtract the mass of F from the total mass of MF2.
Given that the mass of MF2 is 18.69 grams and the molar mass of F is 19.00 grams/mol, we can calculate the grams of M present.
Step 1: Calculate the mass of F in MF2.
The mass of F = (Molar mass of F) * (number of moles of F)
Since we do not know the exact molar mass of M or the number of moles of F, we are unable to calculate the grams of M present in the sample of MF2.
In summary, we were able to determine the number of moles of F in the sample of MF2 but are unable to calculate the grams of M present without knowing the molar mass of M or the number of moles of F.