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2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s)...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s)...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s) + O2(g) → 2Ca0(s) b. C2H4(g) + 302(g) → 2002(g) + 2H,0(9) Data Table Trial 1 Value 8.50 g 100 ml (0.1 L) 21 Deg C 18 Deg C Measured or calculated Quantity Mass NaNO3 weighed out Volume H2O (L) (NaNO3) M Moles of NaNO3 Temperature initial Temperature Final AT (Tf-TI) q of the solution q of the coffee cup qof NaNO3 dissolution AH...
need help with trial 1 EQUATIONS and CALCULATIONS: 1) 2) 3) 4) 5) 6) 7) In...
need help with trial 1
EQUATIONS and CALCULATIONS: 1) 2) 3) 4) 5) 6) 7) In this experiment, we are measuring the q of the surroundings then calculating the q for the system (the dissolution of sodium nitrate, NaNO3, in water) using the equations below. Calculate q for the system, using 4.184 J/g °C) as the specific heat of water, and 1.0 g/mL for density of water. Assume the heat capacity of the coffee-cup is 10.0 J/°C. Calculate the enthalpy...
Using the thermodynamic data given in the procedure, calculate ∆H°, ∆S°, and ∆G for the dissolution...
Using the thermodynamic data given in
the procedure, calculate ∆H°, ∆S°, and
∆G for the dissolution of each salt in Part 1. Use the
initial temperature you recorded in lab for the ∆G
calculation.
Data Table 1 Salt Observations Mass of Salt (g) Volume of Water (ml) 5.0 Initial Final Temperature Temperature (°C) (°C) 1.0173 23.1 21.9 Sodium Chloride completely dissolved, slightly cooler 5.0 1.0233 22.8 15.2 Potassium Chloride completely dissolved, cold to the touch 5.0 0.9824 23.2 30.7 Calcium...
- T 2 31 5 6 Using the thermodynamic data given in the procedure, calculate AH°,...
- T 2 31 5 6 Using the thermodynamic data given in the procedure, calculate AH°, AS, and AG for the dissolution of each salt in Part 1. Use the initial temperature you recorded in lab for the AG calculation. AH (kJ/ S (J/mol K) mol) Salt Observations Volume of Water (ml) 5.0 Mass of Salt (g/ Initial Final Temperature Temperature 411.1 72.12 Sodium Chloride 1.0173 23.1 219 82 NaCl) KCI (5) CaCl (s) Nat(a) 436.7 -795.4 completely dissolved slipy...
Gibb's Free Energy, Entropy, and Spontaneous Reactions Results/Observations Run 2 Run 1 52190.573...
please solve 9-14
Gibb's Free Energy, Entropy, and Spontaneous Reactions Results/Observations Run 2 Run 1 52190.5739 0,003 mol 0.0033 e อ. 250 0.230g 0.0047 m . ง : d043 mol 1. Mass of barium hydroxide octahydrate 2. Moles of barium hydroxide octahydrate 3. Mass of ammonium chloride 4. Moles of ammonium chloride 5. Limiting reagent 6. Initial temperature 7. Final temperature 8. AT 9. Qran 10. ΔΗ 11. Average ΔΗ 12. Predicted sign of AS 13. Calculated AG (from Table...
i just need help on this first question, the others parts are just added information if...
i just need help on this first question, the others parts are
just added information if its needed
1. First, calculate the amount of heat energy, Ical, produced in each reaction using Eq. 1 from the Introduction. Convert Vwater to Mwater using a density value of 1.00 g/mL, and s = 4.18 J/(g•°C). Next, calculate the number of moles of NaNO3 (and NH4Cl) present in each reaction using Eq. 2. Finally, calculate the enthalpy change, AH, for each reaction in...
V. Heat of reaction for NaOH (s) + HCI (aq) → Naci (aq) + H20 ()-dH(net) Direct determination Mas...
need help with calculations
V. Heat of reaction for NaOH (s) + HCI (aq) → Naci (aq) + H20 ()-dH(net) Direct determination Mass NaOH Moles NaOH = moles Mass of HCI solution Final temp. of solution Initial temp. of solution AT solution 30 23 C 4 C AH(net)(Direct) per mole NaOH Calculation Indirect determination Heat of dissolution of NaOH (s) [AH(diss)] Mass NaOH Moles NaOH moles Mass of water Final temp. of solution Initial temp. of solution AT solution AH(diss)-...
b. calculate the molar solubility(s) and from that the Ksp of Ba(OH)2 at 0*c. c. calculate...
b. calculate the molar solubility(s) and from that the Ksp of
Ba(OH)2 at 0*c.
c. calculate the delta G* for the dissolution of Ba(OH)2 from
the Ksp calculated in part b, at 0*c.
Section: Date: Pre-Lab Questions 1. A 10.0 mL sample of Balohi, at Or is itrated with 200 M HCL and 5.22 ml of the acid are used to reach the yellow endpoint. a. Calculate the concentration of OH in the 10.0 mL sample of BalOH) at O'C....
(1 pts) Concentration of standard HCl solution (M) Table view List view Trial 1 Trial 2...
(1 pts) Concentration of standard HCl solution (M) Table view List view Trial 1 Trial 2 Initial burette reading (ml) Final burette reading (mL) Volume of HCl added (mL) Solution temperature (°C) (1pts) Average volume HCl added (mL) (2pts) Concentration of OH (M) (2pts) Concentration of Ca2+ (M) I (2pts) Value of Ksp for Ca(OH)2 An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask....
Data Sheet Experiment 1 (Room Temperature): Temp. of Saturated Borax Solution: 2 c ka HCI Concentration:...
Data Sheet Experiment 1 (Room Temperature): Temp. of Saturated Borax Solution: 2 c ka HCI Concentration: A Trial 2 Trial 1 Volume of borax solution titrated: Initial Burette Reading Final Burette Reading 14.62 m jt.k2 1462 E2 mo Volume of HCl used Moles of HCI used Moles of B&Os(OH)2 present in titrant Concentration of BaOs(OH) in titrant 29 34 A2926 Concentration of Na' in titrant Average Conc. of B4Os(OH)e2 in titrant Op294 Average Conc. of Na in titrant Ksp= KEquilibrium...
2. Calculate ASº for the following reactions, using standard entropy values from Appendix C. a. 2Ca(s) + O2(g) → 2Ca0(s) b. C2H4(g) + 302(g) → 2002(g) + 2H,0(9) Data Table Trial 1 Value 8.50 g 100 ml (0.1 L) 21 Deg C 18 Deg C Measured or calculated Quantity Mass NaNO3 weighed out Volume H2O (L) (NaNO3) M Moles of NaNO3 Temperature initial Temperature Final AT (Tf-TI) q of the solution q of the coffee cup qof NaNO3 dissolution AH...
need help with trial 1
EQUATIONS and CALCULATIONS: 1) 2) 3) 4) 5) 6) 7) In this experiment, we are measuring the q of the surroundings then calculating the q for the system (the dissolution of sodium nitrate, NaNO3, in water) using the equations below. Calculate q for the system, using 4.184 J/g °C) as the specific heat of water, and 1.0 g/mL for density of water. Assume the heat capacity of the coffee-cup is 10.0 J/°C. Calculate the enthalpy...
Using the thermodynamic data given in
the procedure, calculate ∆H°, ∆S°, and
∆G for the dissolution of each salt in Part 1. Use the
initial temperature you recorded in lab for the ∆G
calculation.
Data Table 1 Salt Observations Mass of Salt (g) Volume of Water (ml) 5.0 Initial Final Temperature Temperature (°C) (°C) 1.0173 23.1 21.9 Sodium Chloride completely dissolved, slightly cooler 5.0 1.0233 22.8 15.2 Potassium Chloride completely dissolved, cold to the touch 5.0 0.9824 23.2 30.7 Calcium...
- T 2 31 5 6 Using the thermodynamic data given in the procedure, calculate AH°, AS, and AG for the dissolution of each salt in Part 1. Use the initial temperature you recorded in lab for the AG calculation. AH (kJ/ S (J/mol K) mol) Salt Observations Volume of Water (ml) 5.0 Mass of Salt (g/ Initial Final Temperature Temperature 411.1 72.12 Sodium Chloride 1.0173 23.1 219 82 NaCl) KCI (5) CaCl (s) Nat(a) 436.7 -795.4 completely dissolved slipy...
please solve 9-14
Gibb's Free Energy, Entropy, and Spontaneous Reactions Results/Observations Run 2 Run 1 52190.5739 0,003 mol 0.0033 e อ. 250 0.230g 0.0047 m . ง : d043 mol 1. Mass of barium hydroxide octahydrate 2. Moles of barium hydroxide octahydrate 3. Mass of ammonium chloride 4. Moles of ammonium chloride 5. Limiting reagent 6. Initial temperature 7. Final temperature 8. AT 9. Qran 10. ΔΗ 11. Average ΔΗ 12. Predicted sign of AS 13. Calculated AG (from Table...
i just need help on this first question, the others parts are
just added information if its needed
1. First, calculate the amount of heat energy, Ical, produced in each reaction using Eq. 1 from the Introduction. Convert Vwater to Mwater using a density value of 1.00 g/mL, and s = 4.18 J/(g•°C). Next, calculate the number of moles of NaNO3 (and NH4Cl) present in each reaction using Eq. 2. Finally, calculate the enthalpy change, AH, for each reaction in...
need help with calculations
V. Heat of reaction for NaOH (s) + HCI (aq) → Naci (aq) + H20 ()-dH(net) Direct determination Mass NaOH Moles NaOH = moles Mass of HCI solution Final temp. of solution Initial temp. of solution AT solution 30 23 C 4 C AH(net)(Direct) per mole NaOH Calculation Indirect determination Heat of dissolution of NaOH (s) [AH(diss)] Mass NaOH Moles NaOH moles Mass of water Final temp. of solution Initial temp. of solution AT solution AH(diss)-...
b. calculate the molar solubility(s) and from that the Ksp of
Ba(OH)2 at 0*c.
c. calculate the delta G* for the dissolution of Ba(OH)2 from
the Ksp calculated in part b, at 0*c.
Section: Date: Pre-Lab Questions 1. A 10.0 mL sample of Balohi, at Or is itrated with 200 M HCL and 5.22 ml of the acid are used to reach the yellow endpoint. a. Calculate the concentration of OH in the 10.0 mL sample of BalOH) at O'C....
(1 pts) Concentration of standard HCl solution (M) Table view List view Trial 1 Trial 2 Initial burette reading (ml) Final burette reading (mL) Volume of HCl added (mL) Solution temperature (°C) (1pts) Average volume HCl added (mL) (2pts) Concentration of OH (M) (2pts) Concentration of Ca2+ (M) I (2pts) Value of Ksp for Ca(OH)2 An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask....
Data Sheet Experiment 1 (Room Temperature): Temp. of Saturated Borax Solution: 2 c ka HCI Concentration: A Trial 2 Trial 1 Volume of borax solution titrated: Initial Burette Reading Final Burette Reading 14.62 m jt.k2 1462 E2 mo Volume of HCl used Moles of HCI used Moles of B&Os(OH)2 present in titrant Concentration of BaOs(OH) in titrant 29 34 A2926 Concentration of Na' in titrant Average Conc. of B4Os(OH)e2 in titrant Op294 Average Conc. of Na in titrant Ksp= KEquilibrium...
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