I need help with 11 and 12 please.
Homework Answers
Note: During dissolution entropy always increases. The change is entropy is always + ve.
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I need help with 11 and 12 please.
Data Table Mixture NaCl (s) + H2O (1)...
Mixture ΔT NaCl + H2O -0.2 NaNO3 + H2O -0.9 NaCH3COO + H2O 0.9 Which reactions...
Mixture ΔT NaCl + H2O -0.2 NaNO3 + H2O -0.9 NaCH3COO + H2O 0.9 Which reactions are endothermic? Which are exothermic? What is the sign of enthalpy ΔH in each case? What is the sign of change in Gibbs free energy ΔG for each process in the forward direction? Could you predict the sign for entropy ΔS for these reactions? How could you tell the sign?
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...
When sodium chloride dissolves in water, the ions dissociate: NaCl (s) --> Na+ (aq) + Cl-...
When sodium chloride dissolves in water, the ions dissociate: NaCl (s) --> Na+ (aq) + Cl- (aq) Consider the equation, DG = DH - TDS. For each dissolving process, substitute the signs of DG and DH into the equation and predict the possible sign(s) for the entropy (DS). Explain why you chose this sign(s). Does the sign for entropy change seem to make sense? Explain.
1. Is the dissolution process studied today, NaNO, (s) Na+ (aq) + NO, (aq) spontaneous or...
1. Is the dissolution process studied today, NaNO, (s) Na+ (aq) + NO, (aq) spontaneous or nonspontaneous? How can you tell? What is the sign of AG? 2. Using the class's mean value for AH, and the Gibbs-Helmholtz equation, estimate the value for AS for the dissolution process. (See Calculations section.) 3. Based on your observation about the spontaneity of the reaction and the sign of AH, is the value of AS that you calculated a minimum or a maximum?...
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...
free energy enthal Name Entropy (S) The second factor involved in determining whether or not a...
free energy enthal
Name Entropy (S) The second factor involved in determining whether or not a process is spontaneous is the change in randomness or entropy (AS). Entropy is represented by the symbol S. Again, experience can help us understand the relationship between entropy and spontaneous processes. If we look at the two drawings below, we can predict which picture represents the stack of marbles "before and after they are bumped. We expect the stack of marbles (less random; lower...
QUESTION 1 Heat is required to dissolve NaOH(s) in water. A-True B-False -------------------- QUESTiON 2 The...
QUESTION 1 Heat is required to dissolve NaOH(s) in water. A-True B-False -------------------- QUESTiON 2 The below equation represents an exothermic reaction: Reactants + delta H ----> product ATrue B-False -------------------- QUESTION 3 The Styrofoam cup was used as an insulated device that allows heat loss A-True B-False -------------------- QUESTION 4 The following is an endothermic reaction; NaOH+ HCI------> NaCl+H2O+42.12KJ A-True B-False -------------------- QUESTION 5 NaOH(s)---> Na^+(aq)+CH^-(aq)+44.02kJ Calculate the amount (in moles) of NaOH needed to make the reaction above...
the first photo is the data I collected, can you help me fill the second photo?...
the first photo is the data I collected, can you help me fill
the second photo? third photo is information you might need to do
so.
25
ml of HCl and NaOH each
C. Heat of Reaction Original temp of HCl Onginal terms of No Oth, Final temp. of neutralized 21.5°C 21.8°C 25.2°C 22.1°C 21.6°C 25.5°C Change in temperature, AT (tako average of the original temperatures of HCl and NaOH) quo assume 50 g H20 are present) AH for the...
QUESTION 9 If two reactions are coupled, then 2. A product of one reaction is a...
QUESTION 9 If two reactions are coupled, then 2. A product of one reaction is a reactant of the other, and the overall process is product-favored. b. A product of one reaction is a reactant of the other, and the overall process is reactant-favored C. The heat released from an exothermic reaction is used in an endothermic reaction. The Gibbs free energy released from a product-favored reaction is released to the surroundings. causing an increase in entropy for a second...
please help with 2, 4, 6. thanks!! Activity 4: Observations and Interpretations NHCl(s) + H2O(l) +...
please help with 2, 4, 6. thanks!!
Activity 4: Observations and Interpretations NHCl(s) + H2O(l) + NH(aq) + Cl(aq) 1) What did you observe when you added the concentrated HCl solution to the saturated solution of ammonium chloride? White crystal precipitate formed 2) Interpret the observation in 1, in terms of the equation given above and LeChateliers Principle. 3) What did you observe when you placed this test tube in the boiling water bath? By adding heat, the precipitate went...
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...
1. Is the dissolution process studied today, NaNO, (s) Na+ (aq) + NO, (aq) spontaneous or nonspontaneous? How can you tell? What is the sign of AG? 2. Using the class's mean value for AH, and the Gibbs-Helmholtz equation, estimate the value for AS for the dissolution process. (See Calculations section.) 3. Based on your observation about the spontaneity of the reaction and the sign of AH, is the value of AS that you calculated a minimum or a maximum?...
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...
free energy enthal
Name Entropy (S) The second factor involved in determining whether or not a process is spontaneous is the change in randomness or entropy (AS). Entropy is represented by the symbol S. Again, experience can help us understand the relationship between entropy and spontaneous processes. If we look at the two drawings below, we can predict which picture represents the stack of marbles "before and after they are bumped. We expect the stack of marbles (less random; lower...
the first photo is the data I collected, can you help me fill
the second photo? third photo is information you might need to do
so.
25
ml of HCl and NaOH each
C. Heat of Reaction Original temp of HCl Onginal terms of No Oth, Final temp. of neutralized 21.5°C 21.8°C 25.2°C 22.1°C 21.6°C 25.5°C Change in temperature, AT (tako average of the original temperatures of HCl and NaOH) quo assume 50 g H20 are present) AH for the...
QUESTION 9 If two reactions are coupled, then 2. A product of one reaction is a reactant of the other, and the overall process is product-favored. b. A product of one reaction is a reactant of the other, and the overall process is reactant-favored C. The heat released from an exothermic reaction is used in an endothermic reaction. The Gibbs free energy released from a product-favored reaction is released to the surroundings. causing an increase in entropy for a second...
please help with 2, 4, 6. thanks!!
Activity 4: Observations and Interpretations NHCl(s) + H2O(l) + NH(aq) + Cl(aq) 1) What did you observe when you added the concentrated HCl solution to the saturated solution of ammonium chloride? White crystal precipitate formed 2) Interpret the observation in 1, in terms of the equation given above and LeChateliers Principle. 3) What did you observe when you placed this test tube in the boiling water bath? By adding heat, the precipitate went...
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