Final answer:
The molar enthalpy of solution for the fertilizer urea can be calculated using the equation q=mcΔT. In this case, we have 10.0 g of urea dissolved in 150.0 mL of water. The molar enthalpy of solution is -6751 J/mol.
Step-by-step explanation:
The molar enthalpy of solution for the fertilizer urea can be calculated using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass of the solution, c is the specific heat capacity of the solution, and ΔT is the change in temperature. In this case, we have 10.0 g of urea dissolved in 150.0 mL of water. Assuming the specific heat capacity of the solution is the same as that of pure water (4.184 J/g°C), we can plug in the values to calculate the molar enthalpy of solution.
To find the molar enthalpy of solution, we first need to convert grams of urea to moles. The molar mass of urea is 60.06 g/mol, so 10.0 g of urea is equal to 0.1661 moles. Next, we need to calculate the total mass of the solution, which is the sum of the mass of urea and the mass of water. The density of water is 1 g/mL, so 150.0 mL of water is equal to 150.0 g. Thus, the total mass of the solution is 10.0 g + 150.0 g = 160.0 g.
Now, we can plug in the values into the equation: q = mcΔT = (160.0 g)(4.184 J/g°C)(16.7°C - 20.4°C) = -1121.6 J. The negative value indicates that heat is being released.
Finally, we can calculate the molar enthalpy of solution by dividing the heat released by the moles of urea: -1121.6 J / 0.1661 mol = -6751 J/mol.