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26 Cards in this Set
- Front
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Which of the following statements is/are CORRECT?1. For a chemical system, if the reaction quotient (Q) is greater than K, reactant must be converted to products to reach equilibrium.2. For a chemical system at equilibrium, the forward and reverse rates of reaction are equal.3. For a chemical system at equilibrium, the concentrations of products divided by the concentrations of reactants equals one. |
2 only |
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Indicate the expression for Kp for the reaction below. MgCO3(s) MgO(s) + CO2(g) |
Kp = PCO2 |
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Indicate the balanced chemical reaction that corresponds to the following equilibrium constant expression. |
2 CO(g) + O2(g) 2 CO2(g) |
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Consider the chemical reaction below: CO + Cl2 COCl2 K = 4.6 x 109How do the equilibrium concentration of the reactants compare to the equilibrium concentration of the product? |
They are much smaller. |
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For the reaction PCl3(g) + Cl2(g) PCl5(g) at a particular temperature, Kc = 24.3. Suppose a system at that temperature is prepared with [PCl3] = 0.10 M, [Cl2] = 0.15 M, and [PCl5] = 0.60 M. Which of these statements is true? |
The reaction will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached. |
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At a high temperature, equal concentrations of 0.160 mol/L of H2(g) and I2(g) are initially present in a flask. The H2 and I2 react according to the balanced equation below. H2(g) + I2(g) 2 HI(g)When equilibrium is reached, the concentration of H2(g) has decreased to 0.036 mol/L. What is the equilibrium constant, Kc, for the reaction? |
48 |
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SO2(g) + NO2(g) SO3(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 2.0 moles of SO2 and 2.0 moles of NO2 are placed in a 20. L container, what concentration of SO3 will be present at equilibrium? |
0.081 mol/L |
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For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g) ↔ 2NO(g) + Br2(g), DHºrxn = 30 kJ/mol |
Decrease the temperature. |
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Novelty devices for predicting rain contain cobalt(II) chloride and are based on the following equilibrium and reacts to humidity as follows: CoCl2(s) + 6 H2O(g) « CoCl2·6H2O(s) DH = +25.9 kJ blue pink What color will such an indicator be if rain is imminent? |
Pink |
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The equilibrium constant (Kc) for the following reaction is 6.7 x 10–10 at 630 °C. N2(s) + O2(g) 2 NO(g)What is the equilibrium constant for the reaction below at the same temperature? 1/2 N2(g) + 1/2 O2(g) NO(g) |
2.6 x 10-5 |
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Indicate the expression for Kp for the reaction below. 2NOBr(g) <--> 2NO(g) +Br2(l) |
(Kp) = Pno2 / Pnobr2 |
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Indicate a balanced chemical equation that corresponds to the following equilibrium constant expression. |
PbF2(s) Pb2+(aq) + 2 F–(aq) |
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The dissociation of acetic acid proceeds as follows: HC2H3O2 H+ + C2H3O2- If the equilibrium constant for this reaction is 1.8 x 10-5, how does the equilibrium concentration of HC2H3O2 compare to the equilibrium concentration of H+ + C2H3O2- ? |
HC2H3O2 concentration is much larger. |
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Hydrogen iodide decomposes according to the equation2HI(g) H2(g) + I2(g), for which Kc = 0.0156 at 400ºC.0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium. |
0.220 M |
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For the system SiO2(s) + 4 HF(g) ↔ 4 SiF4(g) + 2 H2O(g) ΔH = 156 kJa shift to produce more SiF4(g) would occur if |
the concentration of HF(g) is increased |
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Indicate a balanced chemical equation that corresponds to the following equilibrium constant expression. |
HNO2(aq) + H2O() NO2–(aq) + H3O+(aq) |
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Which of the following statements is/are CORRECT?1. Product concentrations appear in the numerator of an equilibrium constant expression.2. A reaction favors the formation of products if K >> 1.3. Stoichiometric coefficients are used as exponents in an equilibrium constant expression. |
1, 2, and 3 |
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At 700 K, the reaction 2SO2(g) + O2(g) 2SO3(g) has the equilibrium constant Kc = 4.3 x 106, and the following concentrations are present: [SO2] = 0.010 M; [SO3] = 10.M; [O2] = 0.010 M.Is the mixture at equilibrium? If NOT at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium? |
No, right to left. |
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The brown gas NO2 and the colorless gas N2O4 exist in equilibrium, 2NO2 N2O4. In an experiment, 0.625 mole of N2O4 was introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. The concentration of N2O4 at equilibrium was 0.0750 M. Calculate Kc for the reaction. |
7.5 |
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Consider the following equilibria:Calculate the equilibrium constant for the reactionSO2(g) + NO3(g) ↔ SO3(g) + NO2(g). |
780.11 mol/L |
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Indicate a balanced chemical equation that corresponds to the following equilibrium constant expression. |
NH3(g) 1/2 N2(g) + 3/2 H2(g) |
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The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion --> greatest completion). |
3 < 4 < 1 < 2 |
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The equilibrium constant for the reaction Ni(s) + 4CO(g) Ni(CO)4(g) is 5.0 x 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO)4(g) Ni(s) + 4CO(g)? |
2.0 x 10-5 |
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For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2 NOCl(g) ↔ 2 NO(g) + Cl2(g) DHºrxn = 30 kJ/mol |
Increase the temperature. |
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For the reactionSO2(g) + NO2(g) SO3(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 2.0 moles of SO2 and 2.0 moles of NO2 are placed in a 20. L container, what concentration of SO3 will be present at equilibrium? |
0.081 mol/L |
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Indicate the balanced chemical reaction that corresponds to the following equilibrium constant expression.K = (P O2) (P NO2)4 (P N2O5)2 |
2 N2O5(g) O2(g) + 4 NO2(g) |
