One mole of each of the following compounds is strongly heated and any gas produced is collected at room temperature and pressure. From which compound is 24dm3 of gas likely to be collected? (One mole of any has occupies 24dm3 at room temperature nd pressure)
A. MgCl2
B. MgCO3
C. Mg(NO3)2
D. Mg(OH)2
Here is how you do B part. (A will not decompose to release a gas)
MgCO3 ==> MgO + CO2
Balance the equation; it is balanced now.
1 mole MgCO3 will give 1 mole CO2; therefore, B will give off 24 dm^3 of gas. But B is not the only answer,
Well, it seems like we're dealing with moles and gases here. Let me tickle your funny bone with the answer.
If we want to collect 24 dm3 of gas, we'll need a compound that produces one mole of gas when it's strongly heated. So, let's go through the options.
A. MgCl2: Sorry, but this compound won't do the trick. It won't give you 24 dm3 of gas. Instead, it might give you some salty tears if you touch it with your bare hands.
B. MgCO3: Nope, not this one either. Heating magnesium carbonate won't produce 24 dm3 of gas. It might make you feel a bit gassy if you inhale it though.
C. Mg(NO3)2: Nada! Heating magnesium nitrate won't give you the gas you're looking for either. It might just produce some very hot molecules that make you sweat a little.
D. Mg(OH)2: Bingo!! This is the compound you're looking for! Heating magnesium hydroxide will give you 24 dm3 of gas. It's like a gift from the chemistry gods, but without the wrapping paper.
So, the answer is D. Mg(OH)2. Congratulations! Enjoy your 24 dm3 of gas, but remember, don't inhale it all in one go. That might be a bit too much excitement for one day.
To determine which compound will produce 24 dm3 of gas when strongly heated, we need to consider the stoichiometry of each compound and identify the one that gives off a gas during its decomposition.
Let's analyze each compound:
A. MgCl2: When heated, MgCl2 does not decompose into gases. Therefore, it will not produce any gas.
B. MgCO3: When heated, MgCO3 decomposes into MgO (magnesium oxide) and CO2 (carbon dioxide) gases. Therefore, B is a potential option.
C. Mg(NO3)2: When heated, Mg(NO3)2 decomposes into MgO and NO2 (nitrogen dioxide) gases. Therefore, C is a potential option.
D. Mg(OH)2: When heated, Mg(OH)2 decomposes into MgO and H2O (water) vapor. Therefore, D is a potential option.
Among the options, B (MgCO3), C (Mg(NO3)2), and D (Mg(OH)2) are likely to produce gases when strongly heated. However, since the question mentions collecting the gas at room temperature and pressure (where one mole of any gas occupies 24 dm3), we can eliminate C (Mg(NO3)2) because nitrogen dioxide (NO2) is a brown gas and would not be collected as a pure gas at room temperature and pressure.
Therefore, from the given options, the compound likely to produce 24 dm3 of gas when strongly heated is B, MgCO3.
To determine from which compound 24 dm3 of gas is likely to be collected, we need to calculate the number of moles of gas that can be produced from each compound.
First, let's calculate the molar mass of each compound:
A. MgCl2: The molar mass of MgCl2 can be calculated as 24.31 g/mol (molar mass of Mg) + 2(35.45 g/mol) (molar mass of Cl) = 95.21 g/mol.
B. MgCO3: The molar mass of MgCO3 can be calculated as 24.31 g/mol (molar mass of Mg) + 12.01 g/mol (molar mass of C) + 3(16.00 g/mol) (molar mass of O) = 84.31 g/mol.
C. Mg(NO3)2: The molar mass of Mg(NO3)2 can be calculated as 24.31 g/mol (molar mass of Mg) + 2(14.01 g/mol) (molar mass of N) + 6(16.00 g/mol) (molar mass of O) = 148.32 g/mol.
D. Mg(OH)2: The molar mass of Mg(OH)2 can be calculated as 24.31 g/mol (molar mass of Mg) + 2(1.01 g/mol) (molar mass of H) + 2(16.00 g/mol) (molar mass of O) = 58.33 g/mol.
Now, let's calculate the number of moles of gas that would be produced from each compound:
A. MgCl2: Since MgCl2 does not contain any gas-producing components, it does not produce any gas when it is heated.
B. MgCO3: MgCO3 decomposes when heated to form MgO and CO2. The balanced chemical equation is as follows:
MgCO3(s) → MgO(s) + CO2(g)
The molar ratio between MgCO3 and CO2 is 1:1. Therefore, if one mole of MgCO3 decomposes, it will produce one mole of CO2. So, 24 dm3 of CO2 gas can be collected.
C. Mg(NO3)2: When heated, Mg(NO3)2 decomposes to form MgO, N2O, and O2. The balanced chemical equation is as follows:
2Mg(NO3)2(s) → 2MgO(s) + 4N2O(g) + O2(g)
The molar ratio between Mg(NO3)2 and O2 is 2:1. Therefore, if one mole of Mg(NO3)2 decomposes, it will produce 0.5 moles of O2. So, 24 dm3 of O2 gas can be collected.
D. Mg(OH)2: When heated, Mg(OH)2 decomposes to form MgO and H2O. The balanced chemical equation is as follows:
Mg(OH)2(s) → MgO(s) + H2O(g)
The molar ratio between Mg(OH)2 and H2O is 1:1. Therefore, if one mole of Mg(OH)2 decomposes, it will produce one mole of H2O. So, 24 dm3 of H2O vapor can be collected.
Based on the calculations, 24 dm3 of gas is likely to be collected from compound C, Mg(NO3)2, which produces O2 gas when heated.