The thermal decomposition of 1.6608 g of MgSO4 * H2O produces 1.4446 g of a
product in a well-behaved reaction. There are two possibilities:
1) MgSO4 * H2O(s) -> MgSO4(s) + H2O(g)
2) MgSO4 * H2O(s) -> MgO(s) + SO3(g) + H2O(g)
Complete the following table, and then identify the correct solid product by
comparing the calculated masses of MgSO4 and MgO with the observed mass of
the product.
Formula
Substance Weight Moles Mass (g)
-----------------------------------------------------
MgSO4 * H2O __________ __________ __________
MgSO4 __________ __________ __________
MgO __________ __________ __________
Because the observed mass of the product is 1.4446 g, the product is
__________.
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** HERE'S HOW I COMPLETED THE TABLE **
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Formula
Substance Weight Moles Mass (g)
-----------------------------------------------------
MgSO4 * H2O _138.4____ _0.0120___ _1.6608___
MgSO4 _120.4____ _0.0120___ _1.4446___
MgO __40.31___ _0.0358___ _1.4446___
I'm not sure if I did this correctly if I didn't can someone plz exaplin which part and how to do it
Thank You
You have it. So MgSO4 was the product, because you have to end up with the same number of moles of Mg as you started with.
Well, it looks like you've completed the table correctly! Great job! Now let's analyze the table to determine the correct solid product.
In the table, we calculated the moles and mass (in grams) of each substance based on the given information. The molar masses of MgSO4, H2O, and MgO were used to calculate the moles, and then multiplied by the molar masses to find the corresponding masses.
Looking at the last row of the table, we can see that the calculated mass of MgO is 1.4446 g, which matches the observed mass of the product. This means that the correct solid product is MgO.
So, in conclusion, the correct solid product is MgO. It seems like the clown bot has successfully helped you complete the table and identify the product. Feel free to ask any more questions or if you need further clarification!
Looks like you did a good job completing the table. Let's go through each step to make sure everything is correct:
1. To calculate the weight of MgSO4 * H2O, we use its molar mass: Mg = 24.31 g/mol, S = 32.06 g/mol, O = 16 g/mol, and H = 1 g/mol. Since there is one Mg, one S, four O, and two H atoms in MgSO4 * H2O, the molar mass is:
Weight (MgSO4 * H2O) = (24.31 + 32.06 + (16 * 4) + (1 * 2)) g/mol = 138.4 g/mol
2. As given in the question, 1.6608 g of MgSO4 * H2O is used, so we divide the mass by the molar mass to get the number of moles:
Moles (MgSO4 * H2O) = 1.6608 g / 138.4 g/mol ≈ 0.0120 mol
3. To calculate the weight of MgSO4, we need to subtract the weight of the water from the weight of MgSO4 * H2O. Since the molar mass of water is 18.02 g/mol (H2O = 2 * 1 + 16 = 18), we can calculate:
Weight (MgSO4) = 1.6608 g - (18.02 g/mol * 0.0120 mol) = 1.4446 g
4. The molar mass of MgO is 40.31 g/mol (Mg = 24.31 and O = 16). Since there is one Mg and one O atom in MgO, we can calculate:
Weight (MgO) = 40.31 g/mol * 0.0358 mol = 1.4446 g
5. Based on the observed mass of the product being 1.4446 g, we can compare it with the calculated masses of MgSO4 and MgO.
Looking at the table, we can see that the observed mass matches the calculated mass of MgO (1.4446 g). Therefore, the correct solid product is MgO.
I hope this clarifies the steps and helps you understand the process. If you have any further questions, feel free to ask!
You have correctly started filling in the table for the given information. Let's go through each part of the table:
1) Formula Weight: This represents the molar mass of each substance mentioned in the reaction. The molar mass is calculated by adding up the atomic masses of each element in the formula.
For example:
- The formula weight of MgSO4 * H2O can be calculated as:
Mg: 24.31 g/mol + S: 32.06 g/mol + 4 x O: 16.00 g/mol + 2 x H: 1.01 g/mol + O: 16.00 g/mol = 138.4 g/mol.
- The formula weight of MgSO4 can be calculated as:
Mg: 24.31 g/mol + S: 32.06 g/mol + 4 x O: 16.00 g/mol = 120.4 g/mol.
- The formula weight of MgO can be calculated as:
Mg: 24.31 g/mol + O: 16.00 g/mol = 40.31 g/mol.
2) Moles: This represents the number of moles of each substance in the reaction. To calculate the moles, you can use the formula: Moles = Mass (g) / Formula weight (g/mol).
For example:
- The moles of MgSO4 * H2O can be calculated as: 1.6608 g / 138.4 g/mol = 0.0120 mol.
- The moles of MgSO4 can also be calculated as: 1.4446 g / 120.4 g/mol = 0.0120 mol.
- The moles of MgO can be calculated as: 1.4446 g / 40.31 g/mol = 0.0358 mol.
3) Mass: This represents the calculated mass of each substance based on the number of moles and the formula weight. To calculate the mass, you can use the formula: Mass (g) = Moles x Formula weight (g/mol).
For example:
- The calculated mass of MgSO4 * H2O can be found as: 0.0120 mol * 138.4 g/mol = 1.6608 g (as given).
- The calculated mass of MgSO4 can be found as: 0.0120 mol * 120.4 g/mol = 1.4446 g (as given).
- The calculated mass of MgO can be found as: 0.0358 mol * 40.31 g/mol = 1.4446 g (as given).
By comparing the observed mass of the product (1.4446 g) with the calculated masses, you can determine which substance is the correct solid product. In this case, the calculated mass of MgO matches the observed mass of the product, so the correct solid product is MgO.
Therefore, the correct answer to fill in the last blank is: MgO.