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In the Thermodynamics and Equilibrium lab, you found that the sign of the experimentally determined value...
This is a thermodynamics of urea dissolution lab. Temperature of water was 25.6 C Temperature of...
This is a thermodynamics of urea dissolution lab. Temperature of
water was 25.6 C Temperature of water mixed with urea was 21.7 C
Mass of 25ml of water - 24.5 g Heat capacity of water given: c:
2.184 J/g C Mass of urea is 1.5 g Calculate q and please answer the
questions above. Thanks.
1. Remember for calorimetry that sys - AH' and that you measured surr 2. Calculate AH', using the following equation: 4surr = -Asys 3. The...
How would I go about finishing questions 3-6 for this lab report on thermodynamics? The reaction...
How would I go about finishing questions 3-6 for this lab
report on thermodynamics?
The reaction was the dissolving of KNO3 in water
CRC Handbook. ThermouyilaL Parameter AH" Value from your data. 32.8KT Ima 9.83K AS AG at 25°C 3. Show how you calculated the value for AH from CRC Handbook data. 4. Discuss the meanings of the signs of your values for AH', and AS'. What do they tell you about the process in which potassium nitrate dissolves in...
Can someone help me finish my table? all the inforamtion is there. molarity of HCL =0.5M g...
can someone help me finish my
table? all the inforamtion is there.
molarity of HCL =0.5M
grams of borax = 18.41g
the Relationship between Thermodynamics and Equilibrium 21 Complete the data table for each temperature studied. Beaker Label 42 °C 45 °C 36 ° C 39 °C 33 °C 2EC 138℃-2°C| ーでー 46℃ Temperature reading (C) Absolute temperature (K) 1/T Final buret reading Initial buret reading Volume of HCI Moles of H+ Moles of B Os(OH)2 Molarity of B,Os(OH)2 306.230.2...
I need help answering the rest of these. Experiment TA Lab Team Members Finding Equilibrium Constants:...
I need help answering the rest of these.
Experiment TA Lab Team Members Finding Equilibrium Constants: The Solubility of Borax Report Sheet Part A: Titration of Room Temperature Borax: Kg Molarity of Standard HCl solution: 004 u Temperature of room temperature borate mixture (T); T. in 20.00 Tin 293.15 K Trial 1 LLLLLL Final buret reading HCl, mL Initial buret reading HCI, ml 135.26 12.40 110.48 11.052 Trial 3 Trial 2 (if done) 138.53 39.00 18.83 18.76 110.66 110. 36...
(2pts) Post-lab Questions AH Choose. ΔΗ (1pts) 1. Do you expect the solubility of Borax to...
(2pts) Post-lab Questions AH Choose. ΔΗ (1pts) 1. Do you expect the solubility of Borax to increase or decrease as temperature increases? Select the option that best explains why. A. Solubility will increase, because as Tincreases the term becomes smaller therefore will get larger. B. Solubility will increase, because as Tincreases the IT term becomes smaller therefore K will get smaller. C. Solubility will decrease, because as increases the term becomes smaller therefore Kwill get smaller. D. Solubility will decrease,...
10. When sodium chloride dissolves in water, the ions dissociate: NaCl (s) = Na+ (aq) +...
10. When sodium chloride
dissolves in water, the ions dissociate: NaCl (s) = Na+
(aq) + Cl- (aq)
Write ionic equations, similar to the one above, that describe
how NaNO3 and NaCH3CO2 each
dissociate as they dissolve in water. Include heat as a reactant or
product in each equation.
Here is what I answered:
NaNO3 (s) = Na+ +
NO3- + heat
NaC2H3O2 + Heat =
Na+ +
C2H3O2-(ag)
Lab data table attached to determine where to place heat.
AGO no...
The first two pages are a background of the lab and there is a page with...
The first two pages are a background of the lab and there is a
page with the results. I would appreciate any help with this. If
needed I have the pre-lab questions as well. I added in the pre-lab
questions I will get them answered and updated again if that is
what is needed.
Report Sheet Name Pre-Lab Questions [Ni(H0) ] + + 6 NHỮ[Ni(NH] + + H2O 1. Given the spontaneous chemical reaction shown above and the fact that...
The first two pages are the background of the lab. I would appreciate any help with...
The first two pages are the background of the lab. I would
appreciate any help with the pre-lab questions, even if you cannot
answer them all, so I could continue to the post-lab on my own.
Experiment Thermodynamics: Entropy vs. Enthalpy OH, Background The formation of a Lewis Acid-Base complex occurs when you have a lone pair of electrons being donated to an electropositive ion or atom. Common examples are the Lewis Acid-Base complexes that most metal ions form in...
REPORT BOOK QUESTIONS These questions from the Report Book are included in the manual to help you prepare for the E...
REPORT BOOK QUESTIONS These questions from the Report Book are included in the manual to help you prepare for the Experiment and the Computer Preliminary Exercises. a) Write an equation describing the reaction of HCI with water. b) Hence, write an equation describing the reaction between an aqueous solution of ammonia and hydrochloric acid. Indicate the acid base conjugate pairs. Calculate the energy absorbed by the calorimeter alone, calorimeter Refer to Laboratory Manual, Page Calculate the energy absorbed by the...
i need help with this lab please. can i get someone to answer the entire thing....
i need help with this lab please. can i get someone to answer
the entire thing. thank you
Instructor Equilibria of Coordination Compounds OBSERVATIONS AND DATA 1. The formation of complex ions with ammonia The net ionic equation for the reaction of excess Cuso, with NH, is 24 Cu2+ + 4NH3 [cu (NH3)4] The predicted effect on the reaction above of adding excess NH, (based on Le Châtelier's principle) is The reaction will shift to the night and product formation...
This is a thermodynamics of urea dissolution lab. Temperature of
water was 25.6 C Temperature of water mixed with urea was 21.7 C
Mass of 25ml of water - 24.5 g Heat capacity of water given: c:
2.184 J/g C Mass of urea is 1.5 g Calculate q and please answer the
questions above. Thanks.
1. Remember for calorimetry that sys - AH' and that you measured surr 2. Calculate AH', using the following equation: 4surr = -Asys 3. The...
How would I go about finishing questions 3-6 for this lab
report on thermodynamics?
The reaction was the dissolving of KNO3 in water
CRC Handbook. ThermouyilaL Parameter AH" Value from your data. 32.8KT Ima 9.83K AS AG at 25°C 3. Show how you calculated the value for AH from CRC Handbook data. 4. Discuss the meanings of the signs of your values for AH', and AS'. What do they tell you about the process in which potassium nitrate dissolves in...
can someone help me finish my
table? all the inforamtion is there.
molarity of HCL =0.5M
grams of borax = 18.41g
the Relationship between Thermodynamics and Equilibrium 21 Complete the data table for each temperature studied. Beaker Label 42 °C 45 °C 36 ° C 39 °C 33 °C 2EC 138℃-2°C| ーでー 46℃ Temperature reading (C) Absolute temperature (K) 1/T Final buret reading Initial buret reading Volume of HCI Moles of H+ Moles of B Os(OH)2 Molarity of B,Os(OH)2 306.230.2...
I need help answering the rest of these.
Experiment TA Lab Team Members Finding Equilibrium Constants: The Solubility of Borax Report Sheet Part A: Titration of Room Temperature Borax: Kg Molarity of Standard HCl solution: 004 u Temperature of room temperature borate mixture (T); T. in 20.00 Tin 293.15 K Trial 1 LLLLLL Final buret reading HCl, mL Initial buret reading HCI, ml 135.26 12.40 110.48 11.052 Trial 3 Trial 2 (if done) 138.53 39.00 18.83 18.76 110.66 110. 36...
(2pts) Post-lab Questions AH Choose. ΔΗ (1pts) 1. Do you expect the solubility of Borax to increase or decrease as temperature increases? Select the option that best explains why. A. Solubility will increase, because as Tincreases the term becomes smaller therefore will get larger. B. Solubility will increase, because as Tincreases the IT term becomes smaller therefore K will get smaller. C. Solubility will decrease, because as increases the term becomes smaller therefore Kwill get smaller. D. Solubility will decrease,...
10. When sodium chloride
dissolves in water, the ions dissociate: NaCl (s) = Na+
(aq) + Cl- (aq)
Write ionic equations, similar to the one above, that describe
how NaNO3 and NaCH3CO2 each
dissociate as they dissolve in water. Include heat as a reactant or
product in each equation.
Here is what I answered:
NaNO3 (s) = Na+ +
NO3- + heat
NaC2H3O2 + Heat =
Na+ +
C2H3O2-(ag)
Lab data table attached to determine where to place heat.
AGO no...
The first two pages are a background of the lab and there is a
page with the results. I would appreciate any help with this. If
needed I have the pre-lab questions as well. I added in the pre-lab
questions I will get them answered and updated again if that is
what is needed.
Report Sheet Name Pre-Lab Questions [Ni(H0) ] + + 6 NHỮ[Ni(NH] + + H2O 1. Given the spontaneous chemical reaction shown above and the fact that...
The first two pages are the background of the lab. I would
appreciate any help with the pre-lab questions, even if you cannot
answer them all, so I could continue to the post-lab on my own.
Experiment Thermodynamics: Entropy vs. Enthalpy OH, Background The formation of a Lewis Acid-Base complex occurs when you have a lone pair of electrons being donated to an electropositive ion or atom. Common examples are the Lewis Acid-Base complexes that most metal ions form in...
REPORT BOOK QUESTIONS These questions from the Report Book are included in the manual to help you prepare for the Experiment and the Computer Preliminary Exercises. a) Write an equation describing the reaction of HCI with water. b) Hence, write an equation describing the reaction between an aqueous solution of ammonia and hydrochloric acid. Indicate the acid base conjugate pairs. Calculate the energy absorbed by the calorimeter alone, calorimeter Refer to Laboratory Manual, Page Calculate the energy absorbed by the...
i need help with this lab please. can i get someone to answer
the entire thing. thank you
Instructor Equilibria of Coordination Compounds OBSERVATIONS AND DATA 1. The formation of complex ions with ammonia The net ionic equation for the reaction of excess Cuso, with NH, is 24 Cu2+ + 4NH3 [cu (NH3)4] The predicted effect on the reaction above of adding excess NH, (based on Le Châtelier's principle) is The reaction will shift to the night and product formation...
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