The oxidation of ethanal produced 2.7 g of silver. Calculate how many liters of acetylene were

The oxidation of ethanal produced 2.7 g of silver. Calculate how many liters of acetylene were required to obtain the required mass of ethanal.

Solution:
1. Let’s compose the reaction equations:
С2Н2 + Н2О = Н2С = СНОН = Н3С – СОН – the reaction of acetylene hydration, vinyl alcohol is released, which undergoes isomerization and ethanal is formed;
Н3С – СОН + Ag2O = 2Ag + CH3COOH – oxidation of ethanal, obtained silver and acetic acid:
2. Let’s calculate the number of moles of silver, if its mass is known:
M (Ag) = 107.8 g / mol;
Y (Ag) = m / M = 2.7 / 107.8 = 0.025 mol;
3. Determine the number of moles of ethanal:
X mol (C2H4O) – 0.025 mol (Ag);
-1 mol 2 mol hence, X mol (C2H4O) = 1 * 0.2 = 0.0125 mol;

4. Let’s compose the proportion according to the hydration reaction equation, determine the amount of acetylene moles:
X mol (C2H2) – 0.0125 mol (C2H4O);
-1 mol – 1 mol from here, X mol (C2H2) = 1 * 0.0125 / 1 = 0.0125 mol;
5. Let’s calculate the volume of acetylene according to Avogadro’s law:
V (C2H2) = 0.0125 * 22.4 = 0.28 l.
Answer: it took 0.28 liters to carry out the reaction. acetylene.