How much NH3 can be produce from 20 liter 32,5 wt%(NH2)2CO (urea) aqueous solution. The reaction path way is :
(NH2)2CO +H2O= 2NH3+ CO2
Thanx
Here is a solved example of a stoichiometry problem. Just follow the steps. I assume you know how to convert 32.5 wt% to molarity.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the amount of NH3 that can be produced from a 20-liter 32.5 wt% (NH2)2CO (urea) aqueous solution, you need to follow these steps:
Step 1: Convert the weight percent (wt%) of (NH2)2CO to grams of (NH2)2CO.
- Assuming a 32.5 wt% (NH2)2CO solution, there are 32.5 grams of (NH2)2CO per 100 grams of solution.
- Therefore, in a 20-liter solution, there would be (32.5 grams/100 grams) x (20,000 grams) = 6,500 grams of (NH2)2CO.
Step 2: Calculate the molar mass of (NH2)2CO (urea).
- (NH2)2CO has a molar mass of 60.06 g/mol.
Step 3: Determine the moles of (NH2)2CO in the solution.
- Using the molar mass calculated in the previous step, divide the mass of (NH2)2CO (6,500 grams) by the molar mass of (NH2)2CO (60.06 g/mol).
- Moles of (NH2)2CO = 6,500 grams / 60.06 g/mol = 108.22 mol.
Step 4: Use the stoichiometric ratio from the balanced chemical equation to determine the moles of NH3 produced.
- According to the balanced equation: (NH2)2CO + H2O → 2NH3 + CO2
- 1 mole of (NH2)2CO produces 2 moles of NH3.
- So, the moles of NH3 would be twice the moles of (NH2)2CO: Moles of NH3 = 2 x 108.22 mol = 216.44 mol.
Step 5: Convert the moles of NH3 to liters.
- NH3 is a gas at room temperature and pressure, assuming ideal gas behavior.
- At STP (Standard Temperature and Pressure: 0°C and 1 atm), 1 mole of any ideal gas occupies 22.4 liters.
- Therefore, the volume of NH3 produced would be: 216.44 mol x 22.4 L/mol = 4,845.86 liters.
In conclusion, approximately 4,845.86 liters of NH3 can be produced from a 20-liter 32.5 wt% (NH2)2CO (urea) aqueous solution, based on the given reaction pathway.