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Terms in this set (28)
Solute
what you put in the solvent to create a solution.
Ex: NaCl(s) + H20= NaCl (aq)
Solvent
what a solute is added to in order to create a solution
Solution
solute + solvent
Stock
a concentrated solution that will be diluted to some lower concentrate for use
Molarity Equation
M1V1=M2V2
Reaction rates
the speed of a reaction
Increase in concentration of reactants on reaction rate
an increase in concentration of reactants means there will be more molecules in the same volume of space so there will be more collisions. With more collisions there is a higher probability that there will be collisions with enough force and correct orientations so the rate of reactions will increase.
Molarity
moles of solution per liter of solution
Dilution
lower concentrate from stock
Collision Theory
1. Molecules must collide to react
2. Molecules must collide with enough energy to overcome the energy of activation
3. Molecules must collide with the
correct orientation to form products.
Apply collision theory to explain why increasing the temperature of a reaction usually increases the reaction rate.
If the temperature of a reaction is increased then the molecules have more kinetic energy. More kinetic energy means the molecules are traveling faster. The faster moving molecules will hit more frequently and they will also hit with more force. There will be a greater number of collisions that have the correct orientation and a force greater than the activation energy so the rate of the reaction will increase. The rule of thumb is if you increase the temperature by 10℃ the rate of the reaction will double.
Hydrogen peroxide (H2O2) decomposes to water and oxygen gas more rapidly when manganese dioxide is added. The manganese dioxide is not consumed in the reaction. Explain the role of the manganese dioxide in the reaction.
Manganese dioxide is a catalyst. A catalyst speeds up the rate of a reaction by lowering the activation energy but it is not used up in the reaction. This is illustrated in the energy profile diagram on the below.
Explain why a crushed solid reacts with a gas more quickly than a large chunk of the same solid.
When a solid is crushed there is a larger surface area. With a larger surface area there are more molecules that will be able to react at the same time. With more frequent collisions the probability of the molecules hitting with enough force (E>Ea) and hitting with the correct orientation will increase. So the rate of the reaction will increase.
List the four factors that affect the rate of a reaction:
a. temperature
b. concentration
c. surface
area
d. catalyst
Using the kinetic molecular theory (molecular collisions etc.), explain in your own words how changing surface area affects the rate of a chemical reaction.
Increasing the surface area means that there are more molecules exposed to collisions. Increasing the number of collisions causes there to be a greater number of collisions that have the correct orientation and an energy greater than the activation energy so the rate of the reaction will increase.
Using the Kinetic molecular theory, explain in your own words how increasing the temperature of the reactants affects the rate of a chemical reaction
If the temperature of a reaction is increased then the molecules have more kinetic energy. More kinetic energy means the molecules are traveling faster. The faster moving molecules will hit more frequently and they will also hit with more force. There will be a greater number of collisions and therefore a greater number with correct orientation and enough energy to overcome the activation energy barrier. The greater force also makes it EVEN more likely that the molecules will collide with energy greater than the activation energy. Both of these cause the rate of the reaction to increase.
Using the Kinetic molecular theory, explain in your own words how increasing the concentration of the reactants affects the rate of a chemical reaction.
If we increase the concentration of the reactants there are be more molecules in the same volume so there will be more frequent collisions. With more frequent collisions the probability of the molecules hitting with enough force (E>Ea) and hitting with the correct orientation will increase. So the rate of the reaction will increase.
Increasing the temperature of a reaction by 10℃ approximately doubles the rate of the reaction. What would be the effect of increasing the temperature of a reaction by 20℃?
The rule of thumb is if you increase the temperature by 10℃ the rate of the reaction will double. So if the reaction rate is raised by twenty degrees it will double for the first ten degrees and double that for the second ten degrees so if you raise the temperature of a reaction by 20℃ you will increase the rate by 2X2 or quadruple the rate.
Given the reaction: aA + bB → cC + dD
a. Write the general rate law.
rate = k [A]m [B]n Any letters that are not a, b can be used for the rate orders. (x,y)
Given the reaction: aA + bB → cC + dD
What is the relationship between m and n and a and b?
There is no relationship between m and n (the rate orders) and a and b (the coefficients of the balanced equation). (m≠ a and n≠b)
The values for k, m and n must be determined experimentally.
Given the reaction: aA + bB → cC + dD
What is the rate constant, k, dependent on?
The rate constant takes into account the temperature, the activation energy, and the orientation requirements of the collisions.
What does the size of k indicate about the rate of a reaction?
A large k means a fast reaction rate and a small k means a slow reaction rate.
What is the order of a reaction
Order is the power of each reactant.
Balance the following equations and write the equilibrium
expression for each.
2 H2S(g) ↔ 2 H2(g) + S2(g)
K= (〖[H_2]〗^2 [S_2])/〖[H_2 S]〗^2
Balance the following equations and write the equilibrium expression for each.
2 Na2O2(s) + 2 CO2(g) ↔ 2 Na2CO3(s) + O2(g)
K= ([O_2])/〖[CO_2]〗^2
Solids are never included in an equilibrium expression.
Balance the following equations and
write the equilibrium expression for each.
H2SO4(l) + SO3(g) ↔ H2S2O7(l)
K=1/([SO_3])
Liquids are never included in an equilibrium expression.
what is K
the ration of products to reactants @ equilibrium
What is Q
the ratio of products to reactants @ anytime
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CHEMISTRY
The compound HOCI is known, but the related compound HCIO, with a different order for the atoms in the molecule, is not known. Calculations suggest that the activat ion energy for the conversion HOC! → HCIO is 311 kJ mol^-1 and that for the conversion HCIO → HOC! is 31 kJ mol^-1. Estimate ΔU for the reaction HOC! → HCIO.
Verified answer
PHYSICAL SCIENCE
Sea water is a solution that contains dissolved sodium chloride, dissolved magnesium chloride, and many other dissolved ions. Suppose you have a sample of seawater that contains mud and sand. What is the simplest way to get clear sea water from this mixture? Could you use distillation to separate the sea water from the mud? Explain your answer.
Verified answer
CHEMISTRY
(a) Methane (melting point 91 K) and tetrafluoromethane (melting point 89 K) do not form solid solutions with each other, and as liquids they are only partially miscible. The upper critical temperature of the liquid mixture is 94 K at $x(CF_4) = 0.43$ and the eutectic temperature is 84 K at $x(CF_4) = 0.88.$ At 86 K, the phase in equilibrium with the tetrafluoromethane-rich solution changes from solid methane to a methane-rich liquid. At that temperature, the two liquid solutions that are in mutual equilibrium have the compositions $x(CF_4) = 0.10$ and $x(CF_4) = 0.80.$ Sketch the phase diagram. (b) Describe the phase changes that take place when a liquid mixture of 4.0 mol $B_2H_6$ (melting point 131 K) and 1.0 mol $CH_3OCH_3$ (melting point 135 K) is cooled from 140 K to 90 K. These substances form a compound $(CH_3)_2OB_2H_6$ that melts congruently at 133 K. The system exhibits one eutectic at $x(B_2H_6) = 0.25$ and 123 K and another at $x(B_2H_6)$ = 0.90 and 104 K.
Verified answer
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The reaction between ethyl iodide and hydroxide ion in ethanol $$ (C_2H_5OH) $$ solution, $$ \mathrm { C } _ { 2 } \mathrm { H } _ { 5 } \mathrm { I } ( a l c ) + \mathrm { OH } \quad ( a l c ) \longrightarrow \mathrm { C } _ { 2 } \mathrm { H } _ { 5 } \mathrm { OH } ( l ) + \mathrm { I } ^ { - } ( a l c ) $$ has an activation energy of 86.8 kJ/mol and a frequency factor of $$ 2.10 \times 10 ^ { 11 } M ^ { - 1 } \mathrm { s } ^ { - 1 } $$ Which reagent in the reaction is limiting, assuming the reaction proceeds to completion?
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