The 4.000g sample of M2S3 is converted to MO2 and loses 0.277g.what is the atomic weight of M?
Am stuck
M = atomic mass M
O = atomic mass O
S = atomic mass S
MO2 = molar mass MO2
M2S3 = molar mass M2S3
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M2S3 + 5O2 ==> 2MO2 + 3SO2
4.00.........4.00-0.277 = 3.72
4.00 x (2*MO2/M2S3) = 3.72
4.00 x (2*M+4*amO/2*M + 3*S)
4.00 x (2*M + 64) = 3.72(2*M + 3*96)
Solve for M.
You may want to put in a more accurate number for atomic mass S. Post your work if you get stuck.
To find the atomic weight of M, we need to use the information about the sample conversion and the mass lost.
1. Start by calculating the molar mass of M2S3 and MO2. We can use the atomic masses of the elements to calculate the molar masses.
- M2S3:
- Molar mass of M: X
- Molar mass of S: 32.07 g/mol (atomic mass)
- Molar mass of M2S3: 2M + 3S = 2X + 3(32.07)
- MO2:
- Molar mass of M: X
- Molar mass of O: 16.00 g/mol (atomic mass)
- Molar mass of MO2: M + 2O = X + 2(16.00)
2. Next, use the given information that the sample loses 0.277 g during the conversion from M2S3 to MO2. This mass loss can be attributed to the loss of oxygen:
- Mass loss due to oxygen loss: 0.277 g
- Molar mass of oxygen: 16.00 g/mol (atomic mass)
3. Set up an equation based on the molar mass calculations and the mass loss equation:
2X + 3(32.07) - 0.277 = X + 2(16.00)
In this equation, we set the mass loss equal to the difference in molar masses of M2S3 and MO2, as the loss is due to the loss of oxygen.
4. Simplify and solve the equation:
2X + 96.21 - 0.277 = X + 32.00
Combine like terms:
2X + 95.933 = X + 32.00
Move the X term to one side and the constants to the other side:
2X - X = 32.00 - 95.933
Simplify:
X = -63.933
5. The atomic weight of M is -63.933 g/mol. However, it is important to note that atomic weights cannot be negative. Therefore, there may be an error in the calculations or the given information. Double-check the calculations or review the given data to verify the solution.
To find the atomic weight of M, we need to first determine the number of moles of M2S3 in the 4.000g sample.
1. Calculate the number of moles of M2S3:
The molar mass of M2S3 can be calculated by adding the atomic masses of M (atomic weight of M) and S (atomic weight of S). Let's assume the atomic weight of S is known.
Molar mass of M2S3 = (2 x atomic weight of M) + (3 x atomic weight of S)
2. Calculate the number of moles of M2S3:
Number of moles = Mass of sample / Molar mass of M2S3
Number of moles of M2S3 = 4.000g / Molar mass of M2S3
3. Calculate the number of moles of MO2 using stoichiometry:
Since the conversion of M2S3 to MO2 involves the loss of 0.277g, we need to subtract that from the initial mass.
Mass of MO2 = Mass of M2S3 - Loss of mass (0.277g)
Number of moles of MO2 = Mass of MO2 / Molar mass of MO2
4. Since M2S3 and MO2 have the same number of moles (due to stoichiometry), we can equate the number of moles of M2S3 and MO2 to get the atomic weight of M:
Number of moles of M2S3 = Number of moles of MO2
4.000g / Molar mass of M2S3 = (Mass of MO2 / Molar mass of MO2)
5. Solve for the atomic weight of M:
Rearrange the equation to solve for the atomic weight of M:
Molar mass of M2S3 x (Mass of MO2 / Molar mass of MO2) = 4.000g
(2 x atomic weight of M + (3 x atomic weight of S)) x (Mass of MO2 / Molar mass of MO2) = 4.000g
2 x atomic weight of M + (3 x atomic weight of S) = (4.000g x Molar mass of MO2) / Mass of MO2
atomic weight of M = [(4.000g x Molar mass of MO2) / Mass of MO2 - (3 x atomic weight of S)] / 2
Plug in the known values for the atomic weight of S, Molar mass of MO2, Mass of MO2, and calculate the atomic weight of M using the formula.