Respuesta :
Answer:
The change in temperature = 7.65 °C
Explanation:
Step 1: Data given
10.0 grams of ammonium nitrate dissolves in 100.0 grams of water
Hsoln = 25.7 kJ/mol
Molar mass = 80.04 g/mol
Heat capacity of the solution = 4.2 J
Step 2: Calculate moles ammonium nitrate
Moles = mass / molar mass
Moles = 10.0 grams / 80.04 g/mol
Moles =0.125 moles
Step 3: Calculate q
q = 25.7 kJ/mol * 0.125 moles
q = 3.2125 kJ = 3212.5 J
Step 4: Calculate change in temperature
q = m*c*ΔT
3212.5 J = 100g *4.2 J * ΔT
ΔT= 7.65
The change in temperature = 7.65 °C
Explanation:
The given data is as follows.
Molar mass of ammonium nitrate = 80.0 g/mol
So, we will calculate the number of moles of ammonium nitrate as follows.
No. of moles = [tex]\frac{\text{given mass}}{\text{molar mass}}[/tex]
= [tex]\frac{10.0 g}{80.0 g/mol}[/tex]
= 0.125 mol
Heat released due to solution of ammonium nitrate = [tex]\Delta H \times \text{no. of moles}[/tex]
= [tex]25.7 kJ/mol \times 0.125 mol[/tex]
= 3.2125 KJ
= 3212.5 J (as 1 kJ = 1000 J)
Therefore, calculate the total mass of solution as follows.
mass of solution(m) = (10.0 + 100.0 ) g
= 110.0 g
Hence, heat released will be calculated as follows.
Q = [tex]m \times C \times \Delta T[/tex]
3212.5 J = [tex]110.0 \times 4.2 J \times \Delta T[/tex]
[tex]\Delta T = 6.95^{o}C[/tex]
Thus, we can conclude that the change in temperature of the solution is [tex]6.95^{o}C[/tex].
