For the reaction of ethene, C2H4(g), with oxygen(g) to form carbon dioxide(g) and water(g), what number of moles of carbon dioxide can be produced by the reaction of 5.00 mol ethene and 10.2 mol oxygen?
1. 15.3 mol
2. 10.2 mol
3. 6.80 mol
4. 10.0 mol
5. None of these
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The balanced chemical equation for the reaction is:
C2H4 + 3O2 -> 2CO2 + 2H2O
From the equation, it can be seen that 1 mole of C2H4 reacts with 3 moles of O2 to produce 2 moles of CO2.
So, to find the number of moles of CO2 produced, we need to determine the limiting reactant.
The mole ratio of ethene to oxygen is 1:3, which means that for every mole of ethene, we need 3 moles of oxygen.
Given:
Moles of C2H4 = 5.00 mol
Moles of O2 = 10.2 mol
Using the mole ratio, we can determine the maximum number of moles of CO2 that can be produced if both reactants are completely consumed.
Moles of O2 needed = 3 * Moles of C2H4 = 3 * 5.00 mol = 15.00 mol
Since we have 10.2 mol of O2, which is less than the required 15.00 mol, it means that oxygen is the limiting reactant.
Now, we can determine the number of moles of CO2 produced from the given moles of oxygen:
Moles of CO2 = 2 * Moles of O2 = 2 * 10.2 mol = 20.4 mol
Therefore, the correct answer is:
5. None of these.
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