Answer:
The theoretical yield of urea = <u>120.35kg</u>
The percent yield for the reaction = <u>72.70%</u>
Explanation:
Lets calculate -
The given reaction is -
→
Molar mass of urea 
= 60g/mole
Moles of 
= 
(since 
)
= 4011.76 moles
Moles of 
= 
= 
= 2386.36 moles
Theoritically , moles of required = double the moles of
but , 
, the limiting reagent is
Theoritical moles of urea obtained = 
= 
Mass of 2005.88 mole of =
= 120352.8g
= 120.35kg
Therefore , theroritical yeild of urea = 120.35kg
Now , Percent yeild = 
72.70%
Thus , the percent yeild for the reaction is 72.70%
The molecular weight of H2O is 18g/mol.
Therefore, 27.9 g H2O / (1mol/18g) = 0.155 mol H2O
Calculating only for the latent heat, the heat required to be released for this amount of H2O to condense is:
40.7 kJ/mol (0.155 mol) = 6.3 kJ or -6.3 kJ since it is to be released
Energy released from changing the phase of a substance from the liquid phase to solid phase can be calculated by using the specific latent heat of fusion. The heat of fusion of water at 0 degrees Celsius is 334 J/g. Calculation are as follows:
<span>
Energy = 5 grams x 334 J/g
</span><span>Energy = 1670 J</span>
Answer:
151 g/mol
Explanation:
When a nonvolatile substance is added to a solvent, the freezing point of the solvent is changed, which is called cryoscopy. When temperature change can be calculated by:
ΔT = Kf*W
Where Kf is the molal freezing point constant of the solvent and W is the molality of the solution.
For cyclohexane, Kf = 20.2 °C/molal, and the freezing point is 6.4 °C, so:
6.4 - 1.05 = 20.2 * W
20.2W = 5.35
W = 0.26485 molal
The molality is:
W = m1/m2*M1
Where m1 is the mass of the solute (in g), m2 is the mass of the solvent (in kg), and M1 is the molar mass of the solute. So:
0.26485 = 2.00/0.05M1
0.0132425M1 = 2.00
M1 = 151 g/mol
Answer:THIS IS NOT THE ANSWER
is this for the chemistry A final 10th grade for connexus (unit7 lesson 2)?
Explanation:
