Question

When 10.00 ml of 1.00 m hcl solution is mixed with 115 ml of 0.100 m naoh solution in a constant-pressure calorimeter, the temperature rises from 22.45 °c to 23.25 °
c. calculate q for this reaction, assuming that the heat capacity of the calorimeter is the same as that of 125 g of water.?

Answer 1

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.

Answer 2

The amount of energy required by the reaction is $\boxed{418\,{\text{J}}}$ .

Further Explanation:

Given:

The volume of $HCl$  mixed in the calorimeter is $10.0\,{\text{ml}}$ .

The volume of $NaOH$  mixed in the calorimeter is $115\,{\text{ml}}$ .

The initial temperature of the solution is ${22.45\:^{\circ}\text{C}}$  or $295.6\,{\text{K}}$ .

The final temperature of the solution is ${23.25\:^{\circ}\text{C}}$  or $296.4\,{\text{K}}$ .

The specific heat capacity of water is $4.18\,{{\text{J}}\mathord{\left/{\vphantom{{\text{J}}{{\text{g}}\cdot{\text{K}}}}}\right.\kern-\nulldelimiterspace}{{\text{g}}\cdot{\text{K}}}}$ .

Concept:

The total volume of the calorimeter after the addition of  $HCl$ and $NaOH$  is:

$\begin{aligned}V&=115+10\\&=125\,{\text{ml}}\\\end{aligned}$

The density of the given solution is $1\,{{\text{g}}\mathord{\left/{\vphantom{{\text{g}}{{\text{ml}}}}}\right.\kern-\nulldelimiterspace}{{\text{ml}}}}$ . Therefore, the mass of the solution is:

$\begin{aligned}m&={\text{density}}\times{\text{volume}}\\&=1\,{{\text{g}}\mathord{\left/{\vphantom{{\text{g}}{{\text{ml}}}}}\right.\kern-\nulldelimiterspace}{{\text{ml}}}}\times125\,{\text{ml}}\\&=125\,{\text{g}}\\\end{aligned}$

The change in temperature of the calorimeter is.

$\begin{aligned}\Delta T&={T_f}-{T_i}\\&=296.4-295.6\\&=0.8\\\end{aligned}$

Now, the amount of heat absorbed by the calorimeter to complete the reaction is given as:

$q=m\times C\times\Delta T$

Here,  $q$ is the amount of heat required for the reaction and $C$  is the heat capacity of the calorimeter.

Substitute the values in the above expression.

$\begin{aligned}q&=125\times4.18\times0.8\\&=125\times3.344\\&=418\,{\text{J}}\\\end{aligned}$

Thus, the amount of energy required by the reaction is $\boxed{418\,{\text{J}}}$ .

Learn More:

1. One consequence of the third law of thermodynamics is that brainly.com/question/3564634

2. According to Charles’s law, for a fixed quantity of gas at constant pressure brainly.com/question/7316997

3. Calculate the average translational kinetic energy (sometimes just called average kinetic energy) brainly.com/question/9078768

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.