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2. The equilibrium constant for HI decomposition at 500 °C is 5.8×10-3.
2HI(g)—–> H2(g) + I2(g)
At that temperature reactants and products are gaseous. (There is no change in the total number of moles, so Kc = Kp.) A sample of 0.43 mol of HI is placed in a 1.00 L vessel which is then heated to 500 °C. When equilibrium is reached, what is the molar concentration of H2? (Give units). [H2] =
Iodine is sparingly soluble in pure water. However, it does `dissolve’ in solutions containing excess iodide ion because of the following reaction:
I–(aq) + I2(aq) I3–(aq) K = 710
For each of the following cases calculate the equilbrium ratio of [I3–] to [I2].
a . 5.00×10-2 mol of I2 is added to 1.00 L of 5.00×10-1 M KI solution.
b. The solution above is diluted to 12.00 L.
At a particular temperature, K = 1.00×102 for the reaction:
H2(g) + F2(g) 2HF(g)
In an experiment, at this temperature, 1.90 mol of H2 and 1.90 mol of F2 are introduced into a 1.25-L flask and allowed to react. At equilibrium, all species remain in the gas phase.
What is the equilibrium concentration (in mol/L) of H2?
mol/L
Tries 0/10
What is the equilibrium concentration (in mol/L) of HF?
mol/L
Tries 0/10
To the mixture above, an additional 9.50×10-1 mol of H2 is added. What is the new equilbrium concentration (in mol/L) of HF?
mol/L
Is the statement true or false, with respect to the specified reaction in each case?
•
H2(g) + F2(g) 2HF(g)
If a vessel, containing an equilbrium mixture of these gases, is pressurized by adding helium gas, then the equilibrium position will shift to the left.
TrueFalse
•
H2(g) + F2(g) 2HF(g)
If an equilbrium mixture of these gases is released into a vessel of larger volume, then the equilibrium position will not shift.
TrueFalse
•
Fe3+(aq) + SCN–(aq) FeSCN2+(aq)
If KOH is dissolved in this solution, then the equilibrium position will shift to the left. (Note that Fe(OH)
3 is insoluble.)
TrueFalse
•
H2(g) + I2(g) 2HI(g)
If hydrogen gas is added to an equilbrium mixture of these gases, then the equilibrium position will not shift.
TrueFalse
•
H2O(g) + CO(g) H2(g) + CO2(g) (Exothermic)
If the temperature is increased, then the equilibrium constant for this reaction equation will increase.
TrueFalse
Given:
2CO(g) + O2(g) 2CO2(g)
K = 3.01×1091
C(graphite) + 1/2O2(g) CO(g)
K = 2.28×1023
What is the equilibrium constant for the following reaction?
C(graphite) + O2(g) CO2(g)
Given the following equilibrium constants at 427°C:
O2(g) + 4Na(l) 2Na2O(s)
K1 = 2.50×1049
O2(g) + 2Na(l) 2NaO(g)
K2 = 2.50×109
O2(g) + 2Na(l) Na2O2(s)
K3 = 2.00×1028
O2(g) + Na(l) NaO2(s)
K4 = 3.33×1013
What would be the value of the equilibrium constant for each of the following reactions, at 427°C?
Na2O2(s) + Na(l) NaO(g) + Na2O(s)
Tries 0/10
2NaO2(s) + 2Na(l) 2NaO(g) + Na2O2(s)
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