Answer :
Answer: [tex]\Delta H[/tex] for the reaction is 87935 J
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.
[tex]Molarity=\frac{moles}{\text {Volume in L}}[/tex]
[tex]moles of HCl[/tex]=[tex]Molarity\times {\text {Volume in L}}=1.35\times 0.01=0.135moles[/tex]
[tex]moles of NaOH[/tex]= [tex]Molarity\times {\text {Volume in L}}=1.76\times 0.01=0.176moles[/tex]
As 1 mole of HCl neutralizes 1 mole of NaOH
0.135 moles of HCl will neutralize = 0.135 mole of NaOH
Thus HCl is the limiting reagent.
[tex]Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})[/tex]
Q = Heat absorbed by water = ?
m = mass of water = 200 g (volume of water=200ml, density of wtaer = 1 g/ml)
c = specific heat capacity = [tex]4.18 J/g^0C[/tex]
Initial temperature of water = = 24.6°C
Final temperature of water= = 38.8 °C
[tex]Q=200\times 4.18\times (38.8-24.6)[/tex]
[tex]Q=11871.2J[/tex]
Thus heat released by 0.135 moles is = -11871.2 J
heat released by 1 mole is =[tex]\frac{-11871.2 J}{0.135}\times 1=-87935J[/tex]
The heat of reaction, ΔH is 87935 J
Molarity and Heat of Reaction ΔH
- Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.
- The heat of reaction ΔH, is the amount of heat evolved or absorbed when a chemical reaction occurs between molar quantities of the reactants as represented in the equation of reaction.
Equation of reaction between HCl and NaOH is given below:
- HCl + NaOH ----> NaCl + H₂O
Molarity = number of mole/volume
Number of moles = molarity * volume
Number of moles of HCl = 1.35 M * 0.1 L = 0.135 moles
Moles of NaOH = 1.76 M * 0.1 L = 0.176 moles
1 mole of HCl neutralizes 1 mole of NaOH
- Therefore, 0.135 moles of HCl will neutralize 0.135 mole of NaOH
- Therefore, NaOH is in excess and HCl is the limiting reagent.
Calculating the quantity of heat evolved:
- Q = mcΔT
where m is mass, c is specific heat capacity, ΔT is temperature change
- Quantity of heat evolved by reaction = Heat absorbed by water
Heat absorbed by water, Q = mcΔT
mass of water = density * volume
density of water = 1 g/mL
volume of water = 200 mL
mass of water = 1 g/mL * 200 mL
mass of water = 200 g
specific heat capacity of water, c = 4.18 J/g°C
- ΔT = final temperature of water - initial temperature of water
Initial temperature of water = = 24.6°C
Final temperature of water= = 38.8 °C
ΔT = 38.8 - 24.6 = 13.7°C
Q = 200 g * 4.18 J/g°C * 14.2°c
Q = 11871.2 J
Therefore, heat released by 0.135 moles is = -11871.2 J
Heat released by 1 mole = 11871.2 * 1/0.135
Heat released by 1 mole = 87935 J
Therefore, the heat of reaction, ΔH is 87935 J
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