Topic
Q:
If an endothermic reaction is at equilibrium, how will the equilibrium shift when heat is added to the reaction?
View Available Hint(s)
Q:
If the reaction
is at equilibrium, what direction will the reaction shift if \( \mathrm{NH}_{3} \) gas is added?
View Available Hint(s)
The reaction will shift to produce both reactants and products.
The reaction will shift to produce products.
The reaction will remain unchanged.
The reaction will shift to produce reactants.
Q:
Consider the reaction below. \( \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \leftrightharpoons 2 \mathrm{NH}_{3}(g) \) Which of the following changes would cause less \( \mathrm{NH}_{3} \) to be produced?
View Available Hint(s)
adding \( \mathrm{N}_{2} \)
decreasing the volume
increasing the volume
adding \( \mathrm{H}_{2} \)
Q:
Consider the following equilibrium between \( \mathrm{N}_{2} \mathrm{O}_{4} \) and \( \mathrm{NO}_{2} \).
Which changes would cause the reaction to become darker brown?
Riew Available Hint(s)
Run the reaction at a lower temperature.
Decrease the volume of the container.
Increase the pressure in the reaction vessel.
Q:
Consider the following equilibrium between \( \mathrm{N}_{2} \mathrm{O}_{4} \) and \( \mathrm{NO}_{2} \).
Which changes would cause the reaction to become darker brown?
Riew Available Hint(s)
Run the reaction at a higher temperature.
Q:
92. Write an appropriate Lewis structure for each compound. Make
certain to distinguish between ionic and molecular compounds.
\( \begin{array}{llll}\text { a. } \mathrm{Al}_{2} \mathrm{O}_{3} & \text { b. } \mathrm{ClF}_{5} & \text { c. } \mathrm{MgI}_{2} & \text { d. } \mathrm{XeO}_{4}\end{array} \)
Q:
Predict the effect of decreasing the reaction temperature.
shift right
shift left
no effect
Q:
Predict the effect (shift right, shift left, or no effect) of increasing the reaction temperature.
shift right
shift left
no effect
Q:
Select the correct image. Identify the model that represents a mixture of two compounds.
Q:
An equilibrium mixture of the unbalanced reaction
has
\[ \mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{I}(\mathrm{g}) \]
What is the value of the equilibrium constant?
Express your answer numerically to four decimal places.
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