chemistry Consider the reaction between 50.0 mL liquid methanol, CH_3 OH (densit

Question

chemistry Consider the reaction between 50.0 mL liquid methanol, CH_3 OH (density = 0.850 g/mL), and 22.8 L O_2 at 27 degree C and a pressure of 2.00 atm. The products of the reaction are CO_2 (g) and H_2 O (g). Calculate the number of moles of H_2 O formed if the reaction goes to completion. Urea (H_2 NCONH_2) is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide: 2NH_3 (g) + CO_2 (g) rightarrow^Heat _Pressure H_2 NCONH_2 (s) + H_2 O (g) Ammonia gas at 223 degree C and 90. atm flows into a reactor at a rate of 500. L/min. Carbon dioxide at 223 degree C and 45 atm flows into the reactor at a rate of 600. L/min. What mass of urea is produced per minute by this reaction assuming 100% yield?

Explanation / Answer

Q73.

V = 50 mL of methanol

m = D*V = 0.85g/ml * 50 ml= 42.5 g

mol of methanol = mass/MW = 42.5/32.04 = 1.326466 mol of methanol

V = 22.8 L of O2 at T = 27°C --> 300 K P = 2 atm

mol:

PV = nRT

n = PV/(RT) = 2*22.8 / (0.082*300 ) = 1.8536 moles of O2 gas:

CH3OH + O2 = CO2 + 2H2O

balance

CH3OH + 3/2O2 = CO2 + H2O

moles of H2O formed:

1.326466 ¨--> 3/2*1.326466 = 1.989699 mol of O2 required, which we do not have so;

1.8536 mol of O2 --> 2/3*1.8536 = 1.23573 mol of methanol, which we DO have

so

1.23573 mol of methanol reacts to form --> 1.23573 mol of water

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