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by BlastRoom
Students explain reaction rate using collision energy, orientation, activation energy, and catalysts.
#chemistry
20 questions
One question set, multiple game modes. Tap any game to see it in action. Not sure which to pick?
Answer to place stones and capture territory.
Outrun the snow together.
Earn blasts, then hunt the other team.
Answer to earn energy, then climb.
The class blasts through walls together.
Bid on mystery lots. Most money wins.
Sell tours. Nice, standard, or a total scam.
Answer, restock, and serve the rush.
More correct answers pulls the rope your way.
Answer, then shoot down the alien wave.
Answer, then tap to leap the frozen ridge.
Two reactant particles collide with the correct orientation but bounce apart after a gentle impact. Which explanation best fits collision theory?
A collision between two molecules has energy above the activation energy, but the reactive ends are not lined up. What most likely prevents a reaction?
Which particle event is most likely to produce products in a reaction?
As a reaction proceeds in a closed flask, its rate usually slows down. Which collision-theory explanation fits?
A gas reaction has many molecular collisions each second but still reacts slowly. Which collision-theory explanation fits?
Why does collision orientation matter more for reactions between large molecules than for reactions between single atoms?
A reaction has an activation energy of 50 kJ/mol. A correctly oriented collision supplies 65 kJ/mol. What is the expected result?
For a reaction with activation energy 80 kJ/mol, a collision supplies 80 kJ/mol and has the correct orientation. How should it be classified?
A collision is correctly oriented but supplies 70 kJ/mol for a reaction with activation energy 90 kJ/mol. What happens?
Reaction X has activation energy 45 kJ/mol, and reaction Y has activation energy 110 kJ/mol. At the same temperature, why is X likely faster?
A collision supplies 150 kJ/mol for a reaction with activation energy 120 kJ/mol, but the molecules are badly aligned. What is the best prediction?
An uncatalyzed reaction has activation energy 100 kJ/mol. With a catalyst, the pathway requires 55 kJ/mol. Why does the rate increase?
A catalyst is recovered unchanged after a reaction. What particle-level role did it most likely play?
Which statement best explains how adding a catalyst changes a reacting mixture?
A catalyst is added to a reversible reaction already at equilibrium. Which effect fits collision theory?
A solution reaction speeds up when the concentration of one reactant is doubled. What collision-theory explanation fits?
A powdered solid reacts faster with acid than one large chunk of the same mass. Why?
A reaction mixture is warmed from 20 °C to 40 °C and reacts faster. Which explanation uses collision theory correctly?
A gas-phase reaction speeds up when the container volume is decreased at constant temperature. Why?
Stirring a solid reactant in a liquid often increases the reaction rate. What is the best collision-theory reason?
Crack the passcode before the zombies get in.
Answer, then swat bugs for bonus points.
Race through questions at your own speed.
Same question on every screen. Fastest wins.
Pick a tile, answer, hit bonuses and steals.
Dynamic Equilibrium
20 questions
