The synthesis of urea, commonly used as a fertilizer, is made by reaction of carbon dioxide and ammonia, giving urea (CH4N2O) and water according to the following reaction.CO2(g)  +  2 NH3(g)  →   CH4N2O(s)  +  H2O(l)Data:   compound                   molar mass  (g mol-1)            Carbon dioxide                       44.01            Ammonia                                17.04            Urea                                        60.07            Water                                      18.02Calculate the theoretical yield of urea in grams, starting with 9.66 g ammonia and excess carbon dioxide. Give your answer to three significant figures. Do not include units.

To calculate the theoretical yield of urea, we first need to determine the number of moles of ammonia (NH3) we have.

1. Calculate the number of moles of ammonia: The molar mass of ammonia is given as 17.04 g/mol. We can use this to find the number of moles in 9.66 g of ammonia.

   Number of moles = mass / molar mass Number of moles of NH3 = 9.66 g / 17.04 g/mol = 0.567 mol

2. Determine the stoichiometry of the reaction: From the balanced chemical equation, we can see that the reaction consumes ammonia and produces urea in a 2:1 ratio. This means that for every 2 moles of ammonia consumed, 1 mole of urea is produced.

3. Calculate the number of moles of urea produced: Using the stoichiometry of the reaction, we can calculate the number of moles of urea produced.

   Number of moles of urea = 0.567 mol NH3 * (1 mol CH4N2O / 2 mol NH3) = 0.283 mol CH4N2O

4. Calculate the mass of urea produced: We can now use the molar mass of urea to find the mass of urea produced.

   Mass = number of moles * molar mass Mass of urea = 0.283 mol * 60.07 g/mol = 17.0 g

So, the theoretical yield of urea is 17.0 g.