Time (s) | Temperature (degree celcius) |
0 | 20 |
5 | 24 |
10 | 27.5 |
15 | 27.2 |
20 | 26.9 |
25 | 26.6 |
30 | 26.2 |
35 | 25.9 |
40 | 25.6 |
45 | 25.3 |
50 | 25 |
55 | 24.6 |
60 | 24.3 |
ANSWER
Q, a ) :
ANSWER Q, b ) :
Given:
1. Tmax = 27.5 °C
2. T initial = 24.3 °C
3. ΔT=T2–T1 = (27.5 – 24.3) °C = 3.2 °C
4. The equation for the reaction is
NaOH + HCl → NaCl + H₂O
5. 112.9 g of 1.2915 M NaOH
6. 129.1 g of 1.1294 M HCl
Moles of HCl = n = 112.9 g HCl × 1.2915 mole HCl/1 kg HCl = 0.1458 mol HCl
7. Mass of solution = m = (112.9 + 129.1) g = 242 g
8. C = Negligible or zero
The quantity of heat involved in reaction (Exothermic) are:
qreaction + qsolution + qinstruments used = 0
∆H rxn = qreaction / moles of limiting reactant (here in this case HCl)
heat from neutralization + heat to warm solution + heat to warm calorimeter = 0
q1 + q2 + q3 = 0
nΔH + mcΔT + CΔT = 0
0.1458 mol HCl × ΔH + 0.1458 g × 4.184 J·g⁻¹°C⁻¹ × 3.2 °C + (C = Negligible or zero) = 0
0.1458 mol × ΔH + 1952.08= 0
0.1458 mol × ΔH = -1952.08J
∆H rxn = qreaction / moles of limiting reactant
ΔHrxn =−1952.08 /0.1458 mol = -13388 J/mol = -13.39 kJ/mol
ΔHrxn = -13388 J/mol = -13.39 kJ/mol of HCl
ANSWER Q, c ) :
Given:
1. Tmax = 27.5 °C
2. T initial = 24.3 °C
3. ΔT=T2–T1 = (27.5 – 24.3) °C = 3.2 °C
4. The equation for the reaction is
NaOH + HCl → NaCl + H₂O
5. 112.9 g of 1.2915 M NaOH
6. 129.1 g of 1.1294 M HCl
Moles of NaOH = n = 129.1 g NaOH × 1.1294 mole NaOH /1 kg NaOH = 0.1458 mol HCl
7. Mass of solution = m = (112.9 + 129.1) g = 242 g
ΔHrxn =−1952.08 /0.1458 mol of NaOH = -13388 J/mol = -13.39 kJ/mol of NaOH
ΔHrxn = -13388 J/mol = -13.39 kJ/mol of NaOH
ANSWER Q, d ) :
Given:
1. Tmax = 27.5 °C
2. T initial = 24.3 °C
3. ΔT=T2–T1 = (27.5 – 24.3) °C = 3.2 °C
4. The equation for the reaction is
NaOH + HCl → NaCl + H₂O
5. 112.9 g of 1.2915 M NaOH
6. 129.1 g of 1.1294 M HCl
Moles of NaOH = n = 129.1 g NaOH × 1.1294 mole NaOH /1 kg NaOH = 0.1458 mol HCl
7. Mass of solution = m = (112.9 + 129.1) g = 242 g
8. heat to equipments used = heat to warm calorimeter + heat to warm thermometer + heat to warm alumminium stirrer
9. heat to equipments used = (s = 1.131 J/g °C x 30 g) + (s = 0.840 J/g °C x 20 g) = (s = 0.900 J/g °C x 10 g) = 59.73 J/°C
heat from neutralization + heat to warm solution + heat to warm calorimeter + heat to warm thermometer + heat to warm alumminium stirrer = 0
heat from neutralization + heat to warm solution + heat to warm calorimeter = 0
q1 + q2 + q3 = 0
nΔH + mcΔT + CΔT = 0
0.1458 mol HCl × ΔH + 0.1458 g × 4.184 J·g⁻¹°C⁻¹ × 3.2 °C + 59.73 J°C⁻¹ × 3.2 °C = 0
0.1458 mol × ΔH + 373.11= 0
0.1458 mol × ΔH = -373.11J
∆H rxn = qreaction / moles of limiting reactant
ΔHrxn =−373.11/0.1458 mol of NaOH = -2559.05 J/mol = -2.256 kJ/mol of NaOH
ΔHrxn = -2559.05 J/mol = -2.256 kJ/mol of NaOH
ANSWER Q, e ) :
ΔHrxn = literature value of Neutralization reaction is -55.9 kJ/mol which is far away from
ΔHrxn = -13388 J/mol = -13.39 kJ/mol of NaOH . When we consider value for heat of instruments (Calorimeter, Thermometer & Stirrer) large difference is there as they absorbed all raction heat and changed ΔHrxn value. Although system is closed but evolved heat is transfered into closed environment components till equilibrium.
ΔHrxn = -2559.05 J/mol = -2.256 kJ/mol of NaOH
EXPERIMENT 8 HEATS OF REACTION 4. In a neutralization reaction in a well-insulated calorimeter. 112.9 g...
6.A 12.8 g sample of ethanol (C,H,OH) is burned in a calorimeter with a heat capacity of 5.65 kJ/°C. Assume the heat from the sample is negligible compared to the calorimeter. Determine the initial temperature of the calorimeter if the final temperature is 85.7°C. The molar mass of ethanol is 46.07 g/mol. С-Н,ОН , + 3 О,ее — 2 СОде + 3 Н,0 qrxn -1235 kJ 7. Two solutions, initially at 24.60 °C, are mixed in a coffee cup calorimeter...
Thermometer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Ignition wires heat sample Stirrer Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. Water In the laboratory a student burns a 0.568-g sample of tridecanedioic acid (C13H2404) in a bomb calorimeter containing 1080. g...
Thermometer Ignition wires heat sample Stirrer A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.6531 g sample of para-benzoquinone (CH402) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.130x10 g of water. During the combustion the temperature increases from 24.60 to 27.48°C. The heat capacity of water is 4.184 J glock Water The...
2. When 2.0 g of NaOH were dissolved in 53.0 g water in a calorimeter at 24.0°C, the temperature of the solution went up to 33.7°C. Why? Is this solution reaction exothermic? а. b. Calculate qH2o using Eq. 1 Find AH for the reaction as it occurred in the calorimeter (Eq. 5). с. Find AH for the solution of 1.00 g NaOH in water d. J/g Find AH for the solution of one mole NaOH in water. е. J/mol Given...
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.405x103 JK. Ignition wires heat sample Stirrer (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify...
Enthalpy Determination for HCI+NaOH Reaction 1. Mass of empty Styrofoam cup, g: 2. Mass of Styrofoam cup + HCl, g: 3. Initial temperature of HCl solution, "C: Final temperature of solution after mixing, °C 4. 5. Change in temperature, °C: 1215 6. Mass of Styrofoam cup with HCI and NaOH added, g 7. Mass of solution, g: 8. AH of reaction, J: 9. AH of reaction, kJ/mole: 10. AH of reaction based on AH? data, kJ/mole: 11. Percent deviation: Enthalpy...
Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter This is known as calibrating the calorimeter In the laboratory a student burns a 0.319-g sample of phenanthrene (C14H10 in a bomb calorimeter containing 1070. g of water....
- + 0/0.1 points | Previous Answers 3/4 Submissions Used thermometer stirrer coffee cups containing reaction mixture When a 6.14-9 sample of solid iron(II) chloride dissolves in 55.6 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 20.00 °C to 35.10 °C. Calculate AH in kJ/mol FeCl2 for the solution process. FeCl2(s) → Fe2+ (aq) + 2Cl(aq) The specific heat of water is 4.18 J/g-K. AHsolution = 80.445598 x kJ/mol FeCl2.
A common laboratory reaction is the neutralization of an acid with a base. When 49.6 mL of 0.500 M HCl at 25.0°C is added to 52.0 mL of 0.500 M NaOH at 25.0°C in a coffee cup calorimeter (with a negligible heat capacity), the temperature of the mixture rises to 28.2°C. What is the heat of reaction per mole of NaCl (in kJ/mol)? Assume the mixture has a specific heat capacity of 4.18 J/(g·K) and that the densities of the...
RMy Not 14. 0/4 Submissions Used -/0.1 points thermometer stirrer coffee cups containing reaction mixture When a 7.66-g sample of solid iron(III) chloride dissolves in 53.8 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 21.00 oC to 48.44 °C. Calculate AH in kJ/mol FeCl3 for the solution process. FeCl3(s) Fe3+(aq) + 3 CI'(aq) The specific heat of water is 4.18 J/g-K. kJ/mol FeCl3. AHsolution