Respuesta :
We can use the formula
q = m cp ΔT
The
cp of water is 4.18 J/g K
q = 125 (4.18) (23.25 - 22.45)
q = 418 J
The heat evolved for the neutralization reaction is equal to 418 J.
q = m cp ΔT
The
cp of water is 4.18 J/g K
q = 125 (4.18) (23.25 - 22.45)
q = 418 J
The heat evolved for the neutralization reaction is equal to 418 J.
The amount of energy required by the reaction is [tex]\boxed{418\,{\text{J}}}[/tex] .
Further Explanation:
Given:
The volume of [tex]HCl[/tex] mixed in the calorimeter is [tex]10.0\,{\text{ml}}[/tex] .
The volume of [tex]NaOH[/tex] mixed in the calorimeter is [tex]115\,{\text{ml}}[/tex] .
The initial temperature of the solution is [tex]{22.45\:^{\circ}\text{C}}[/tex] or [tex]295.6\,{\text{K}}[/tex] .
The final temperature of the solution is [tex]{23.25\:^{\circ}\text{C}}[/tex] or [tex]296.4\,{\text{K}}[/tex] .
The specific heat capacity of water is [tex]4.18\,{{\text{J}}\mathord{\left/{\vphantom{{\text{J}}{{\text{g}}\cdot{\text{K}}}}}\right.\kern-\nulldelimiterspace}{{\text{g}}\cdot{\text{K}}}}[/tex] .
Concept:
The total volume of the calorimeter after the addition of [tex]HCl[/tex] and [tex]NaOH[/tex] is:
[tex]\begin{aligned}V&=115+10\\&=125\,{\text{ml}}\\\end{aligned}[/tex]
The density of the given solution is [tex]1\,{{\text{g}}\mathord{\left/{\vphantom{{\text{g}}{{\text{ml}}}}}\right.\kern-\nulldelimiterspace}{{\text{ml}}}}[/tex] . Therefore, the mass of the solution is:
[tex]\begin{aligned}m&={\text{density}}\times{\text{volume}}\\&=1\,{{\text{g}}\mathord{\left/{\vphantom{{\text{g}}{{\text{ml}}}}}\right.\kern-\nulldelimiterspace}{{\text{ml}}}}\times125\,{\text{ml}}\\&=125\,{\text{g}}\\\end{aligned}[/tex]
The change in temperature of the calorimeter is.
[tex]\begin{aligned}\Delta T&={T_f}-{T_i}\\&=296.4-295.6\\&=0.8\\\end{aligned}[/tex]
Now, the amount of heat absorbed by the calorimeter to complete the reaction is given as:
[tex]q=m\times C\times\Delta T[/tex]
Here, [tex]q[/tex] is the amount of heat required for the reaction and [tex]C[/tex] is the heat capacity of the calorimeter.
Substitute the values in the above expression.
[tex]\begin{aligned}q&=125\times4.18\times0.8\\&=125\times3.344\\&=418\,{\text{J}}\\\end{aligned}[/tex]
Thus, the amount of energy required by the reaction is [tex]\boxed{418\,{\text{J}}}[/tex] .
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Answer Details:
Grade: High School
Subject: Physics
Chapter: Heat and Thermodynamics
Keywords:
10 ml of 1.00 m HCl, 115 ml of 0.100 m NaOH, constant pressure, calorimeter, heat capacity, same as 125g of water, temperature rises, energy required.
