Experiment B: Data Input Form Heat of reaction for Mg + 2HCl = Heat of reaction...
Experiment B: Data Input Form
Heat of reaction for Mg + 2HCl =
Heat of reaction for MgO + 2HCl =
Heat of formation for H2O= -285.8
Enthalpy of formation for MgO =
Homework Answers
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Experiment B: Data Input Form
Heat of reaction for Mg + 2HCl =
Heat of reaction...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
m this experiment, you will use Hess's Law to determine a heat of reaction that would...
m this experiment, you will use Hess's Law to determine a heat of reaction that would be difficult obtain by direct measurement -- the heat of combustion of magnesium ribbon. The reaction is represented by the equation: D (4) Mg(s) + 1/2O2(g) MgO(s) o bruno solo sbagol i 100) o motorolyobog a n This equation can be obtained by combining, in some way, equations (1), (2), and (3) ob o temo bodo (1) MgO(s) + 2HCl aq) MgCl2(aq) + H2O(1)...
Specific heat = 4.18 J/g*C MgO(s) + 2HCl(aq) → 2Cl(aq) + Mg(aq) + H2O(l): AH = A student added 0.250 g of Mg...
Specific heat = 4.18 J/g*C
MgO(s) + 2HCl(aq) → 2Cl(aq) + Mg(aq) + H2O(l): AH = A student added 0.250 g of MgO(s) to 45.0 mL HCI@ 22.0'C. The temp of the calorimeter rose to 23.5°C. What is qarin kJ? What is the AH in kJ/mol of Mgo for this reaction? Density HCI = 1.05 g/mL
a) Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------>...
a) Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol, calculate the percent error
Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) ...
Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: (0.25 pt.) Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol,...
BG35.2 Enthalpy of Formation of Mgo Page 9 of 12 PRELAB QUESTIONS 1. Read the writeup through the Data Analysis section. A student carried out the experiment described there. The student used 0...
BG35.2 Enthalpy of Formation of Mgo Page 9 of 12 PRELAB QUESTIONS 1. Read the writeup through the Data Analysis section. A student carried out the experiment described there. The student used 0.4894 g of Mg in the first reaction and found that the temperature of the solution went from 22.1 to 42.7'C. In the second reaction, 0.803 g of MgO was used and the solution went from 22.7 to 28.7°C. Calculate the following (show the calculations beside and/or below...
Experiment 19 DATA AND CALCULATIONS Reaction 1 (MgO) Reaction 2 (Mg) 1. Volume of 1.00 M...
Experiment 19 DATA AND CALCULATIONS Reaction 1 (MgO) Reaction 2 (Mg) 1. Volume of 1.00 M HCl 2. Final temperature, t 3. Initial temperature, 4. Change in temperature, ar 2 eC 5. Mass of solid 6. Heat, q kJ 7. AH 8. Moles mol Mgo mol Mg 10. Determine ??mol Mg for reaction (4)". 11. Percent error
Reaction 2 (Ma Reaction 1 (Mgo) 1. Volume of 1.00 M HCT 2. Final temperature, t 3. Initial temper...
please help fill in data table and answer questions.
please show all work. thank you!
Reaction 2 (Ma Reaction 1 (Mgo) 1. Volume of 1.00 M HCT 2. Final temperature, t 3. Initial temperature, t, EO.O ml 50.0 mt 28 a0 oc 4. Change in temperature, t 5. Mass of solid 203 MgO 6. Heat, q k.J kJ kJ k.I 8. Moles mol Mg mol MgO 9. ΔΗ/mol kJ/mol kJ/mol 10. Determine ΔΗ/mol Mg for reaction (4). (10.) II. Percent...
Date DATA Reaction 1 (Mgo) Reaction 2 (Mg) T. Volume of 1.00 M HCI 2. Final temperature, t 3. Ini...
Please help fill in data table and answer questions.
thank you!
Date DATA Reaction 1 (Mgo) Reaction 2 (Mg) T. Volume of 1.00 M HCI 2. Final temperature, t 3. Initial temperature, t 50.0 m 50.0 mL Bc -C 20.8 C 4. Change in temperature, t 5. Mass of solid 6. Heat, q 7. ΔΗ 8. Moles mol Mgo mol Mg kJ/mol kJ/mol 10. Determine ΔH/mol Mg for reaction (4)" (10.) 11. Percent error Outside of lab, you must print...
1. For this reaction in parts A and B, calculate the heat of the reaction using...
1. For this reaction in parts A and B, calculate the heat of the
reaction using the following:
qrxn= -(MC^T + Ccal^T)
Ccalorimeter = 11.6 J/1*C
---------help answer rest if can :)----------
DATA FOR Part A.
Trial #
1
2
3
Mass of calorimeter
41.582 g
41.601 g
41.605 g
Mass of calorimeter+acid
68.857 g
66.832 g
70.596 g
Temperature(C) (acid)
22.0
21.6
21.8
Mass of weighboat
0.703 g
0.704 g
0.701 g
Mass of Mg+weighboat
0.768 g
0.752 g...
m this experiment, you will use Hess's Law to determine a heat of reaction that would be difficult obtain by direct measurement -- the heat of combustion of magnesium ribbon. The reaction is represented by the equation: D (4) Mg(s) + 1/2O2(g) MgO(s) o bruno solo sbagol i 100) o motorolyobog a n This equation can be obtained by combining, in some way, equations (1), (2), and (3) ob o temo bodo (1) MgO(s) + 2HCl aq) MgCl2(aq) + H2O(1)...
Specific heat = 4.18 J/g*C
MgO(s) + 2HCl(aq) → 2Cl(aq) + Mg(aq) + H2O(l): AH = A student added 0.250 g of MgO(s) to 45.0 mL HCI@ 22.0'C. The temp of the calorimeter rose to 23.5°C. What is qarin kJ? What is the AH in kJ/mol of Mgo for this reaction? Density HCI = 1.05 g/mL
BG35.2 Enthalpy of Formation of Mgo Page 9 of 12 PRELAB QUESTIONS 1. Read the writeup through the Data Analysis section. A student carried out the experiment described there. The student used 0.4894 g of Mg in the first reaction and found that the temperature of the solution went from 22.1 to 42.7'C. In the second reaction, 0.803 g of MgO was used and the solution went from 22.7 to 28.7°C. Calculate the following (show the calculations beside and/or below...
Experiment 19 DATA AND CALCULATIONS Reaction 1 (MgO) Reaction 2 (Mg) 1. Volume of 1.00 M HCl 2. Final temperature, t 3. Initial temperature, 4. Change in temperature, ar 2 eC 5. Mass of solid 6. Heat, q kJ 7. AH 8. Moles mol Mgo mol Mg 10. Determine ??mol Mg for reaction (4)". 11. Percent error
please help fill in data table and answer questions.
please show all work. thank you!
Reaction 2 (Ma Reaction 1 (Mgo) 1. Volume of 1.00 M HCT 2. Final temperature, t 3. Initial temperature, t, EO.O ml 50.0 mt 28 a0 oc 4. Change in temperature, t 5. Mass of solid 203 MgO 6. Heat, q k.J kJ kJ k.I 8. Moles mol Mg mol MgO 9. ΔΗ/mol kJ/mol kJ/mol 10. Determine ΔΗ/mol Mg for reaction (4). (10.) II. Percent...
Please help fill in data table and answer questions.
thank you!
Date DATA Reaction 1 (Mgo) Reaction 2 (Mg) T. Volume of 1.00 M HCI 2. Final temperature, t 3. Initial temperature, t 50.0 m 50.0 mL Bc -C 20.8 C 4. Change in temperature, t 5. Mass of solid 6. Heat, q 7. ΔΗ 8. Moles mol Mgo mol Mg kJ/mol kJ/mol 10. Determine ΔH/mol Mg for reaction (4)" (10.) 11. Percent error Outside of lab, you must print...
1. For this reaction in parts A and B, calculate the heat of the
reaction using the following:
qrxn= -(MC^T + Ccal^T)
Ccalorimeter = 11.6 J/1*C
---------help answer rest if can :)----------
DATA FOR Part A.
Trial #
1
2
3
Mass of calorimeter
41.582 g
41.601 g
41.605 g
Mass of calorimeter+acid
68.857 g
66.832 g
70.596 g
Temperature(C) (acid)
22.0
21.6
21.8
Mass of weighboat
0.703 g
0.704 g
0.701 g
Mass of Mg+weighboat
0.768 g
0.752 g...
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