Question

A student reacted 100.0 mL of 0.9800 M HCl with 100.0 mL of 0.9900 M NH3....

A student reacted 100.0 mL of 0.9800 M HCl with 100.0 mL of 0.9900 M NH3. The density of                          
the reaction mixture was 1.02 g/mL and the heat capacity was 4.016 J/g K.                          
Calculate the enthalpy of neutralization by plotting and using the data shown below.

Time(min) Temp(oC)
0.0 23.25
0.5 23.27
1.0 23.28
1.5 23.30
2.0 23.30
3.0 23.35
4.0 23.44
4.5 23.47
mix ---------
5.5 28.75
6.0 28.50
7.0 28.55
8.0 28.48
9.0 28.32
10.0 28.25
11.0 28.20
12.0 28.05
13.0 27.96
14.0 27.80
15.0 27.75

Using the data provided in the excel file, show all of your work for the following calculations:

a.) mean temperature of unmixed reagents (oC)

b.) δελταT from graph (oC)

c.) q absorbed by reaction mixture (J)

d.) q absorbed by calorimeter, stirrer, and thermometer (J)

e.) q total absorbed (J)

f.) q total released (J)

g.) calculation to show limiting reagent

h.) deltaH neutralization for the reaction (kJ/mole of acid)

Homework Answers

Answer #1

a) Average temperature of unmixed reagents is obtained by extrapolating temperature data of 0 to 4.5min at 5min, which is Tinitial = 23.5C

b) DT = Tfinal - Tinitial.

Tfinal data is also obtained by extrrapolation at 5min of temperature data from 5.5min to 15min. Tfinal = 29C

DT = 29-23.5 = 5.5C

c) q absorbed by reaction mixture, q = m*c*DT

Volume of mixture, V = 100+100=200ml. Mass of mixture, m = density*V=1.02*200=204gm

Specific heat, c = 4.016J/(g K).

q = 204*4.016*5.5=4506J

d) , e) and f) Cannt be determined as the heat capacity data for calorimeter system is not available

g) HCl is limiting reagent as its concentration is less than NH3 and both have same volume.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
When a neutralization reaction was carried out using 100.0 mL of 0.7890 M NH3 and 100.0...
When a neutralization reaction was carried out using 100.0 mL of 0.7890 M NH3 and 100.0 mL of 0.7940 M acetic acid, ∆T was found to be 4.76oC. The specific heat of the reaction mixture was 4.104 J g-1 K-1 and its density was 1.03 g/mL. The calorimeter constant was 3.36 J K-1. Show all work below for the following calculations: a.) heat absorbed by the reaction mixture b.) heat absorbed by the calorimeter c.) total heat absorbed d.) number...
You drop 0.050 g of Mg chips into 100.0 mL of 1.00 M HCl and the...
You drop 0.050 g of Mg chips into 100.0 mL of 1.00 M HCl and the temperature of the solution increases from 22.21 °C to 24.46 °C. Assume that cs (solution) - 4.20 J/g °C and that the density of the solution is 1.00 g/mL. What is the enthalpy of the reaction per mole of Mg? Mg (s) + 2 HCl (aq) ----> H2 (g) + MgCl2 (aq)
When a chemist mixed 3.60 g of LiOH and 180. mL of 0.65 M HCl in...
When a chemist mixed 3.60 g of LiOH and 180. mL of 0.65 M HCl in a constant-pressure calorimeter, the final temperature of the mixture was 25.4°C. Both the HCl and LiOH had the same initial temperature, 20.8°C. The equation for this neutralization reaction is: LiOH(s) + HCl(aq) ? LiCl(aq) + H2O(l). Given that the density of each solution is 1.00 g/mL and the specific heat of the final solution is 4.1801 J/g·K, calculate the enthalpy change for this reaction...
When 1.3584 g of sodium acetate trihydrate was mixed into 100.0 mL of 0.2000 M HCl...
When 1.3584 g of sodium acetate trihydrate was mixed into 100.0 mL of 0.2000 M HCl (aq) at 25˚C in a coffee-cup calorimeter, its temperature fell by 0.397˚C. The reaction occurring is as follows: H3O+(aq) + NaCH3CO23 H2O (s) Na+ (aq) + CH3COOH (aq) + 4H2O() a) The heat capacity of the calorimeter is 91.0 J/˚C. Determine the enthalpy of reaction (in kJ/mol). Describe any assumptions that you made. b) Determine the standard enthalpy of formation for the solid sodium...