Volume (mL) | 18.30 |
Temp (C) | 25.849 |
Mass of KNO3 = 7.0056 g
A. Calculate the [K+] for the data entered in the table above for Trial 6.
[K+]: ________ mol/L
B. Calculate the [NO3-] for the data entered in the table above for Trial 6.
[NO3-]: _______ mol/L
C. Calculate the Ksp for Trial 6.
Ksp Trial 6: _________
D. Calculate the ln Ksp for Trial 6.
ln Ksp Trial 6: __________
E. Calculate the 1/T for Trial 6. **Where the value of T is in Kelvin.
Temperature Trial 6: __________ K
1/T: __________
F. Calculate delta G in J/mol for Trial 6.
delta G Trial 6: _________ J/mol
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Volume (mL) 18.30 Temp (C) 25.849 Mass of KNO3 = 7.0056 g A. Calculate the [K+]...
Measurement 1 2 3 4 5 6 Volume (mL) 7.75 9.99 12.00 13.98 16.00 18.30 Temperature (C) 67.580 50.725 42.422 35.551 30.563 25.849 Mass of KNO3 7.0056g 11. Calculate the [K+] for the data entered in the table above for Trial 5. [K+] ______mol/L 12. Calculate the [NO3-] for the data entered in the table above for Trial 5. [NO3-] _____mol/L 13. Calculate the Ksp for Trial 5. [K+] __________ [NO3-] ______- Ksp Trial 5_________- 14. Calculate the ln Ksp...
Measurement 1 2 3 4 5 6 Volume (mL) 7.75 9.99 12.00 13.98 16.00 18.30 Temperature (C) 67.580 50.725 42.422 35.551 30.563 25.849 Mass of KNO3 7.0056g 11. Calculate the [K+] for the data entered in the table above for Trial 3. [K+] ______mol/L 12. Calculate the [NO3-] for the data entered in the table above for Trial 3. [NO3-] _____mol/L 13. Calculate the Ksp for Trial 3. [K+] __________ [NO3-] ______- Ksp Trial 3 _________- 14. Calculate the ln...
Measurement 1 2 3 4 5 6 Volume (mL) 7.75 9.99 12.00 13.98 16.00 18.30 Temperature (C) 67.580 50.725 42.422 35.551 30.563 25.849 Mass of KNO3 7.0056g 11. Calculate the [K+] for the data entered in the table above for Trial 3. [K+] ______mol/L 12. Calculate the [NO3-] for the data entered in the table above for Trial 3. [NO3-] _____mol/L 13. Calculate the Ksp for Trial 3. [K+] __________ [NO3-] ______- Ksp Trial 3 _________- 14. Calculate the ln...
Measurement 1 2 3 4 5 6 Volume (mL) 7.75 9.99 12.00 13.98 16.00 18.30 Temperature (C) 67.580 50.725 42.422 35.551 30.563 25.849 Mass of KNO3 7.0056g 11. Calculate the [K+] for the data entered in the table above for Trial 2. [K+] ______mol/L 12. Calculate the [NO3-] for the data entered in the table above for Trial 2. [NO3-] _____mol/L 13. Calculate the Ksp for Trial 2. [K+] __________ [NO3-] ______- Ksp Trial 2 _________- 14. Calculate the ln...
Measurement 1 2 3 4 5 6 Volume (mL) 7.75 9.99 12.00 13.98 16.00 18.30 Temperature (C) 67.580 50.725 42.422 35.551 30.563 25.849 Mass of KNO3 7.0056g 11. Calculate the [K+] for the data entered in the table above for Trial 4. [K+] ______mol/L 12. Calculate the [NO3-] for the data entered in the table above for Trial 4. [NO3-] _____mol/L 13. Calculate the Ksp for Trial 4. [K+] __________ [NO3-] ______- Ksp Trial 4 _________- 14. Calculate the ln...
Fill in the data sheet and please show your work for the
calculations
Thermodynamics of Potassium nitrate dissolving in water
KNO3(s) ↔
K+ (aq) +
NO3-(aq
Determine the thermodynamic variables, ΔG, ΔH, and ΔS, for the
dissolving of KNO3 in water. You will find these
variables by creating a Van’T Plot, which is a graph of
lnK(sp) vs 1/T.
A set amount of KNO3 is weighed and dissolved in 25mL
of water and heated until all the KNO3 is
dissolved....
the date you need is: 2.0 grams of KNO3, the temp was
22.1.
extra information that might help if you need it: I added 5 mL
of water to the 2.0 g of KNO3.
please answer the 3 parts of the question. Thanks.
Grams KNO,Cryst. Temp, °c 22.1 2.0 g Type your calculation for solubility (in grams KNO,/100 grams water) using the data for the 2.0 gram sample. Type your calculation for molality of KNO, (in mol KNO3/kg water) using...
Data And Report Submission - Entropy Of Borax Dissolution(2pts) "Enthalpy and Entropy Changes of Dissolving Borax"Are you completing this experiment online?YesData CollectionRecord the concentration of HCl used in the experiment (M)0.500Table 1. Data Collection ~60°C trial~50°C trial~40°C trial~30°C trial~20°C trialActual temp (°C)60.350.939.629.518.2Vol. borate solution (mL)5.005.005.014.974.95Initial buret reading (mL)4.9020.9131.7137.8641.50Final buret reading (mL)20.9131.7137.8641.5043.44(14pts) Calculations and AnalysisUse the data collected in the table above to complete the calculations in the following table.Table view List viewTable 2. Calculations ~60°C trial~50°C trial~40°C trial~30°C trial~20°C trialVol. of HCl used (mL)Moles...
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...
Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 44.1 g of KNO3 is dissolved in 221 g of water at 23.00 °C. KNO3(s) to K+ (aq) + NO3- (aq) The temperature of the resulting solution decreases to 21.20 °C. Assume the resulting solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was released by the solution? How much heat was released...