The molar mass of acetaldehyde (CH3CHO) is:
12.011 + 3(1.008) + 12.011 + 15.999 = 44.053 g/mol
Thus, the number of moles of acetaldehyde used is:
23.780 g / 44.053 g/mol = 0.540 mol
From the balanced chemical equation, we see that 2 moles of acetaldehyde produce 2 moles of acetic acid:
2CH3CHO + O2 → 2HC2H3O2
Therefore, the number of moles of acetic acid produced is also 0.540 mol.
The molar mass of acetic acid (HC2H3O2) is:
1.008 + 2(12.011) + 3(15.999) = 60.052 g/mol
So the mass of acetic acid produced is:
0.540 mol x 60.052 g/mol = 32.436 g
Rounded to three significant figures, the answer is:
32.4 g
Therefore, the closest option is 32.428 g.
23.780 g of acetaldehyde (CH3CHO) reacts completely with oxygen to produce acetic acid (HC2H3O2) using manganese (II) acaetate catalyst according to the equation shown below:
2CH3CHO + O2 → 2HC2H3O2
What mass of acetic acid was produced? (Atomic mass: C-12.011 g/mol; 0-15.999 g/mol; H-1.008 g/mol).
32.368 g
32.428 g
64.736 g
64.856 g
1 answer
6 answers