Worksheet 15 (Gen Chem) Chemical Equilibrium 15. Kp for the following reaction is 0.16 at 25...
Consider the following system at equilibrium where Kc = 6.50×10-3 and H° = 16.1 kJ/mol at 298 K. 2 NOBr (g) 2 NO (g) + Br2 (g) The production of NO (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. adding NOBr . 5. removing Br2 .
QUESTION 1 11 poin Given the following endothermic reaction, predict which way the reaction will shift to re-establish equilibrium after being disturbed by each action below 2A) + 3 Bad Cam + 2DG) Removing some C A Toward the reactant side Adding more B. The reaction will not shift in response to the action - Adding more C. The reaction will shift, but there is not enough information to determine which way it was shift - Removing Toward the product...
6. For the following reaction at equilibrium, which change will cause the equilibrium to shift to the left? sle . 2NOBr(g) = 2NO(g) + Br2(g) AH®rxn = 30 kJ/mol A) Decrease the temperature.se (0.5 pt) B) Increase the temperature. C) Increase the container volume. D) Remove some NO. E) Add more NOBr. DOLDS F) Remove some Br2.
The equilibrium constant, Kp, for the following reaction is 6.25 at 298 K. 2NO(g) + Br2(g) 2NOBr(g) If ΔH° for this reaction is -16.1 kJ, what is the value of Kp at 187 K? Kp =
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 19.9 L container at 298K contains NOBr at a pressure of 0.297 atm and NO at a pressure of 0.251 atm, the equilibrium partial pressure of Br2 is ? atm.
Assume the reaction 3 O2(g) <===> 2 O3(g) (Delta H° =285 kJ/mol) is at equilibrium. What effect will each of the following have (explain each)? a) adding more O2 b) adding more O3 c) removing O3 d) increasing pressure in the container e) adding an inert gas f) increasing the temperature in the container
1) Determine the effect of each of the following changes on the equilibrium mixture for the following reaction: N2(g) + O2(g) + 90.2 kJ + 2NO(g) Circle an answer for each change. a. Increasing the temperature Shift to reactants No change Shift to products b. Adding a catalyst Shift to reactants No change Shift to products c. Removing nitrogen monoxide gas Shift to reactants No change Shift to products d. Decreasing the volume of the container Shift to reactants No...
QUESTION 1 The following reaction is endothermic. Which change will shift the equilibrium to the right? 2 503(9) = 2 SO2(g) + O2(9) removing SO3 adding SO2 none of the other answers are correct decreasing the volume (increasing the pressure) decreasing the temperature w
In the endothermic reaction 2NOBr(g) = 2NO(g) + Br2(g) at equilibrium, which of the following changes will result in an increase in the partial pressure of NOBr? 1. decreasing the partial pressure of Br2 II. increasing the size of the reaction vessel III. lowering the overall temperature of the reaction IV. adding a catalyst V. adding He(g) O A I and II I and II O B lland III O c IV and V IV and V III and V...
Which of the following equilibria will shift towards the formation of more products if the reaction at equilibrium is compressed into half its volume? 1. 2N2O(g) + 2N2(g) + O2(g) II. 2CO(g) + O2(g) = 2CO2(g) III. N2(g) + O2(g) + 2NO(g) Both II and III. All three reactions will shift towards the formation of more products. Consider the following reaction at equilibrium. CO2(g) + 2 H2O(l) = CH2(g) + 2O2(g) AH° = +890 kJ Which two of the following...