To determine the molar heat (ΔH) of the solution in kJ/mol, we can use the formula:
ΔH = q / n
where ΔH is the molar heat of the solution in kJ/mol, q is the heat absorbed/released by the solution in Joules, and n is the number of moles of solute.
First, let's calculate the heat absorbed/released by the solution (q):
q = m × c × ΔT
where q is the heat absorbed/released in Joules, m is the mass of the solution in grams, c is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature in °C.
mass of the solution = mass of ammonium nitrate + mass of water = 1.0 g + 50.0 g = 51.0 g
ΔT = final temperature - initial temperature = 23.32°C - 25.0°C = -1.68°C
Now we can calculate q:
q = 51.0 g × 4.18 J/g°C × -1.68°C = -360.2184 J
Next, let's calculate the number of moles of ammonium nitrate (n):
Using the molar mass of NH4NO3:
NH4NO3 = 1(14.007) + 4(1.007) + 1(14.007) + 3(16.00)
NH4NO3 = 28.013 + 4.028 + 14.007 + 48.00
NH4NO3 = 94.050 g/mol
n = mass of ammonium nitrate / molar mass of ammonium nitrate
n = 1.0 g / 94.050 g/mol = 0.01063 mol
Finally, let's calculate the molar heat (ΔH):
ΔH = q / n
ΔH = -360.2184 J / 0.01063 mol = -33923.71 J/mol ≈ -33.92 kJ/mol
Therefore, the molar heat of the solution is approximately -33.92 kJ/mol.
when 1.0g of ammonium nitrate, NH4NO3, dessolves in 50.0g of water, the temprature of the water drops from 25.0c to 23.32c. what is the molar heat (H) of the solution i kj/mol
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