Respuesta :
Hey there!:
moles of AgNO3 = 100 x 0.1 / 1000 = 0.01
moles of NaCl = 100 x 0.200 / 1000 = 0.02
volume of solution = 100 + 100 = 200 mL
mass of solution = 200 x 1 = 200 g
temperature rise = 25.30 - 24.60 = 0.70ºC
Therefore:
Q = m* Cp* ΔT + Cp* ΔT =
200* 4.184 * 0.70 + 15.5 * 0.70 =
Q = 596.61 J
Given the reaction:
Q = 596.61 J
NaCl(aq) + AgNO3(aq)--------> AgCl(s) + NaNO3(aq)
1 mole NaCl ------ 1 mole AgNO3 ------ 1 mole AgCl
0.02 moles NaCl ----- 0.01 moles AgNO3
So:
ΔH = - Q / T
ΔH = - 596.61 * 10⁻³ / 0.01
ΔH = - 59.66 kJ
Hope that helps!
The standard heat of reaction for the given question is ΔH = - 59.66 kJ
From the question, we are given that
Initial temperature, T₁ = 24.6
Final temperature, T₂ = 25.3
Specific heat capacity, Cp = 15.5
to start with, we say that
the number of moles of AgNO₃ = 100 × [tex]\frac{0.1}{1000}[/tex] = 0.01
the number of moles of NaCl = 100 × [tex]\frac{0.2}{1000}[/tex] = 0.02
If we then add up the volume of solutions given to us, we get
100 + 100 = 200 mL
From the question again, we are told that the mass of solution 200g
We know from theory that the change in temperature, ΔT=
ΔT = T₂ - T₁
ΔT = 25.30 - 24.60
ΔT = 0.70ºC
And finally, we apply the formula
Q = (m × Cp × ΔT) + (Cp × ΔT) =
Q = (200 × 4.184 × 0.70) + (15.5 × 0.70) =
Q = 585.76 + 10.85
Q = 596.61 J
The chemical reaction for the question is
NaCl(aq) + AgNO₃(aq) --> AgCl(s) + NaNO₃(aq)
From the equation above, we can conclude that 1 mole NaCl = 1 mole AgNO₃ = 1 mole AgCl
This also means that, 0.02 moles NaCl will react with 0.01 moles AgNO₃
With that established, we can then adjudge that
ΔH = - Q / T
ΔH = - [tex]\frac{596.61 * 10^-3}{0.01 }[/tex]
ΔH = - 59.66 kJ
for more explanation, visit https://brainly.com/question/16720480
