| Rates of Reaction | Potential Energy Diagrams | Table I | Entropy and Spontaneitiy | Equilibrium |
| 10 | 10 | 10 | 10 | 10 |
| 20 | 20 | 20 | 20 | 20 |
| 30 | 30 | 30 | 30 | 30 |
| 40 | 40 | 40 | 40 | 40 |
| 50 | 50 | 50 | 50 | 50 |
| Final Question | ||||
For a collision to be effective, the molecules must hit with enough energy and ________________________.
For a collision to be effective, the molecules must hit with enough energy and ________________________.
spatial orientation
A decrease in temperature would _______________ the rate of a reaction.
A decrease in temperature would _______________ the rate of a reaction.
decrease
Adding a catalyst speeds up a reaction by ______________ the activation energy.
Adding a catalyst speeds up a reaction by ______________ the activation energy.
lowering
Which reacts faster with 1.0 M HCl: 1g chunk of zinc or 1g of zinc powder and why?
Which reacts faster with 1.0 M HCl: 1g chunk of zinc or 1g of zinc powder and why?
1g zinc powder b/c more surface area
What will react faster: ionic solids dissolved in water or covalent solids dissolved in water?
What will react faster: ionic solids dissolved in water or covalent solids dissolved in water?
ionic solids dissolved in water
The amount of energy to get from the reactants to the activated complex
The amount of energy to get from the reactants to the activated complex
activation energy
If the products have more energy than the reactants, the reaction is: exo or endo?
If the products have more energy than the reactants, the reaction is: exo or endo?
endothermic
The difference between the potential energy of the products and the reactants is called
The difference between the potential energy of the products and the reactants is called
heat of reaction
Which particle is at the top of the hill
Which particle is at the top of the hill
activated complex
When a catalyst is added it provides a(n) _______________ pathway for the reaction to occur.
When a catalyst is added it provides a(n) _______________ pathway for the reaction to occur.
alternate/new
Is the formation of C2H2 exo or endothermic?
Is the formation of C2H2 exo or endothermic?
endothermic
Is the decomposition of Al2O3 exo or endothermic?
Is the decomposition of Al2O3 exo or endothermic?
endothermic
When the equation for forming C2H6 is re-written, which side would the heat be included on?
When the equation for forming C2H6 is re-written, which side would the heat be included on?
the right
How would the dissolving of NaCl feel? What would happen to the temperature?
How would the dissolving of NaCl feel? What would happen to the temperature?
feels cold, temperature decreases
How many kJ of heat are released when 10 moles of Al react with oxygen to form Al2O3?
How many kJ of heat are released when 10 moles of Al react with oxygen to form Al2O3?
8377.5 kJ released (H = -8377.5 kJ)
Define entropy.
Define entropy.
disorder/randomness/chaos
Name a phase change that would be a decrease in entropy.
Name a phase change that would be a decrease in entropy.
gas to liquid to solid
Sublimation would be a(n) ____________ in entropy.
Sublimation would be a(n) ____________ in entropy.
increase
Does entropy increase or decrease in the following reaction? C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g)
Does entropy increase or decrease in the following reaction? C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g)
increase
For a reaction to always be spontaneous, the entropy must _____________ and the energy must ______________.
For a reaction to always be spontaneous, the entropy must _____________ and the energy must ______________.
increase, decrease
At equilibrium, rates of the forward and reverse reactions are _______________ and the concentrations of reactants and products are ______________.
At equilibrium, rates of the forward and reverse reactions are _______________ and the concentrations of reactants and products are ______________.
equal, constant
There is phase equilibrium for H2O(s) <--> H2O(l) at what temperature in K?
There is phase equilibrium for H2O(s) <--> H2O(l) at what temperature in K?
273 K
A ___________________ solution is at equilibrium.
A ___________________ solution is at equilibrium.
saturated
When pressure is increased on a chemical reaction at equilibrium, the reaction shifts to the side with _______________________.
When pressure is increased on a chemical reaction at equilibrium, the reaction shifts to the side with _______________________.
less moles of gas
Adding a catalyst (will/will not) shift equilibrium.
Adding a catalyst (will/will not) shift equilibrium.
will not
Explain, in terms of LeChatelier's Principle, why decreasing the concentration of N2 causes a decrease in NO concentration for the following equation. N2 + O2 <--> 2NO
Explain, in terms of LeChatelier's Principle, why decreasing the concentration of N2 causes a decrease in NO concentration for the following equation. N2 + O2 <--> 2NO
The reaction shifts to the left, decreasing the product NO.
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