Answer each of the following questions, and show all your work and final answer in significant figures, where applicable. 1. Consider the following equilibrium system- C(s) + CO2(g) 2C0(g) AH = +120 kJ Indicate the shift in equilibrium, if any, for each of the following scenarios: a) Adding CO2(g) b) Adding C c) Lowering the temperature d) Increasing pressure e) Adding a catalyst 2. At a certain temperature, Ke = 3 for the reaction NO3(g) NO(g) + O2(g) Find the direction of the reaction if at some point in time in a 1.0 vessel the following respective concentrations were measured; [NO] = 2.0 mol/L, [O2] = 1.0 mol/L and NO3(g) = 0.75 mol/L,
Answer each of the following questions, and show all your work and final answer in significant figures, where applicable. 1. Consider the following equilibrium system- C(s) + CO2(g) 2C0(g) AH = +120 kJ Indicate the shift in equilibrium, if any, for each of the following scenarios: a) Adding CO2(g) b) Adding C c) Lowering the temperature d) Increasing pressure e) Adding a catalyst 2. At a certain temperature, Ke = 3 for the reaction NO3(g) NO(g) + O2(g) Find the direction of the reaction if at some point in time in a 1.0 vessel the following respective concentrations were measured; [NO] = 2.0 mol/L, [O2] = 1.0 mol/L and NO3(g) = 0.75 mol/L,
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Chapter1: Chemical Foundations
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![Answer each of the following questions, and show all your work and final answer
in significant figures, where applicable.
1. Consider the following equilibrium system-
C(s) + CO2(g)
2C0(g)
AH = +120 kJ
Indicate the shift in equilibrium, if any, for each of the following scenarios:
a) Adding CO2(g)
b) Adding C
c) Lowering the temperature
d) Increasing pressure
e) Adding a catalyst
2. At a certain temperature, Ke = 3 for the reaction
NO3(g)
NO(g) +
O2(g)
Find the direction of the reaction if at some point in time in a 1.0 vessel the
following respective concentrations were measured; [NO] = 2.0 mol/L,
[O2] = 1.0 mol/L and NO3(g) = 0.75 mol/L,
3. At T = 25°C, K, = 171.3 for the general reaction
2A(g)
B(g)
20(g) + 2D(g)
Calculate Ke.
4. At a certain temperature, Kę = 8 for the reaction
2NO2(g)
NO3(g) +
NO(g)
If 5.0 mol of NO2(g) were added to a 1.0L vessel, calculate the equilibrium
concentrations of all the compounds.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc46def1d-7af4-439c-8152-94ccbbef7e87%2Fa94af291-465b-4de1-adca-a244fa5f5e45%2Fttr50pp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Answer each of the following questions, and show all your work and final answer
in significant figures, where applicable.
1. Consider the following equilibrium system-
C(s) + CO2(g)
2C0(g)
AH = +120 kJ
Indicate the shift in equilibrium, if any, for each of the following scenarios:
a) Adding CO2(g)
b) Adding C
c) Lowering the temperature
d) Increasing pressure
e) Adding a catalyst
2. At a certain temperature, Ke = 3 for the reaction
NO3(g)
NO(g) +
O2(g)
Find the direction of the reaction if at some point in time in a 1.0 vessel the
following respective concentrations were measured; [NO] = 2.0 mol/L,
[O2] = 1.0 mol/L and NO3(g) = 0.75 mol/L,
3. At T = 25°C, K, = 171.3 for the general reaction
2A(g)
B(g)
20(g) + 2D(g)
Calculate Ke.
4. At a certain temperature, Kę = 8 for the reaction
2NO2(g)
NO3(g) +
NO(g)
If 5.0 mol of NO2(g) were added to a 1.0L vessel, calculate the equilibrium
concentrations of all the compounds.
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