For the reaction of ethene, C2H4(g), with oxygen(g) to form carbon dioxide(g) and water(g), how many grams of carbon dioxide could be produced from 2.0 g of ethene and 3.1 g of oxygen?
a. 6.4 g
b. 2.8 g
c. 4.3 g
d. 6.3 g
e. None of these
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To solve this problem, we first need to write out the balanced chemical equation for the reaction:
C2H4 + O2 -> CO2 + H2O
From the equation, we can see that the mole ratio between C2H4 and CO2 is 1:1. This means that for every 1 mole of C2H4, we will produce 1 mole of CO2.
To find the number of moles of C2H4 in 2.0 g, we can use the molar mass of C2H4:
Molar mass of C2H4 = 2(12.01 g/mol) + 4(1.01 g/mol) = 28.05 g/mol
Number of moles of C2H4 = mass of C2H4 / molar mass of C2H4 = 2.0 g / 28.05 g/mol = 0.071 mol
Since the mole ratio between C2H4 and CO2 is 1:1, we will produce 0.071 mol of CO2.
Now, we need to find the mass of 0.071 mol of CO2:
Molar mass of CO2 = 12.01 g/mol + 2(16.00 g/mol) = 44.01 g/mol
Mass of CO2 = number of moles of CO2 * molar mass of CO2 = 0.071 mol * 44.01 g/mol = 3.124 g
Therefore, the maximum mass of carbon dioxide that could be produced from 2.0 g of ethene and 3.1 g of oxygen is 3.124 g.
The correct answer is e. None of these.
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