The balanced equation tells us that 2 moles of acetaldehyde react with 1 mole of oxygen to produce 2 moles of acetic acid.
First, we need to convert the mass of acetaldehyde given to moles:
23.780 g CH3CHO * (1 mol CH3CHO/44.053 g CH3CHO) = 0.54 mol CH3CHO
Next, we use the mole ratio from the equation to determine the moles of acetic acid produced:
0.54 mol CH3CHO * (2 mol HC2H3O2/2 mol CH3CHO) = 0.54 mol HC2H3O2
Finally, we convert the moles of acetic acid produced to grams:
0.54 mol HC2H3O2 * (60.052 g HC2H3O2/1 mol HC2H3O2) = 32.414 g HC2H3O2
Rounding to three significant figures, the mass of acetic acid produced is 32.4 g. Therefore, the correct answer is 32.368 g.
23.780 g of acetaldehyde (CH3CHO) reacts completely with oxygen to produce acetic acid (HC2H3O2) using manganese (II) acetate catalyst according to the equation shown below:
2CH3CHO + O2 → 2HC2H3O2
What mass of acetic acid (HC2H3O2) was produced? (Atomic mass: C-12.011 g/mol; 0-15.999 g/mol; H-1.008 g/mol).
32.428 g
64.736 g
64.856 g
32.368 g
1 answer
1 answer