2NH3 + CO2 = CH4N2O + H2O
How much Urea is produced from 11.4 grams of carbon dioxide with an excess of ammonia.
how many moles in 11.4g of CO2?
The equation says you will get that many moles of urea. Convert to grams.
okay thank you
To find out how much urea is produced from 11.4 grams of carbon dioxide, we need to begin by balancing the chemical equation and then use stoichiometry.
The balanced equation is:
2NH3 + CO2 -> CH4N2O + H2O
From the balanced equation, we can see that the mole ratio between CO2 and CH4N2O is 1:1. Therefore, if we can determine the number of moles of CO2, we can directly calculate the number of moles of CH4N2O produced.
First, we need to convert the grams of CO2 to moles. To do this, we need to know the molar mass of CO2. The molar mass of carbon is approximately 12.01 g/mol, and oxygen is approximately 16.00 g/mol. Adding these up, we get:
12.01 g/mol + (2 x 16.00 g/mol) = 44.01 g/mol
Now we can calculate the number of moles of CO2:
moles of CO2 = mass of CO2 / molar mass of CO2
moles of CO2 = 11.4 g / 44.01 g/mol
Next, we use the mole ratio from the balanced equation to find the moles of CH4N2O produced. From the balanced equation, the ratio is 1:1 between CO2 and CH4N2O.
moles of CH4N2O = moles of CO2
Finally, we can convert the moles of CH4N2O to grams by multiplying the number of moles by the molar mass of CH4N2O. The molar mass of CH4N2O is approximately 60.06 g/mol.
mass of CH4N2O = moles of CH4N2O x molar mass of CH4N2O
Now you can plug in the values into the equations and calculate the amount of urea produced.