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Kinetics and Stoichiometry
Kinetics and Stoichiometry
25
Chemistry
10th Grade
05/03/2011

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Cards

Term
The study of reaction speeds is called
Definition
Kinetics
Term
A catalyst speeds up a chemical reaction by
Definition
lowering the activation energy of the reaction.
Term
If product molecules have a lower energy than reactant molecules, the reaction is (exothermic / endothermic)
Definition
exothermic
Term
The energy of a molecule is stored in its
Definition
bonds
Term
Powdered magnesium will react faster than a strip of magnesium ribbon because
Definition
The powdered magnesium exposes more surface area during the reaction.
Term
A chemical reaction can be slowed down by (increasing / decreasing) temperature.
Definition
decreasing
Term
A chemical that speeds up a chemical reaction is called a
Definition
catalyst
Term
A biological catalyst is called a(n)
Definition
enzyme
Term

[image]

 

The activation energy of the catalyzed reaction is

Definition
10 kJ
Term
True / False:  By speeding up a chemical reaction, you increase the amount of product produced. 
Definition
False.  You don't make any more product; you just create the same amount of product faster.
Term
Increasing the concentration of a reactant speeds up a chemical reaction because
Definition
there will be more frequent collisions between the reactants
Term
A slow-release medicine capsule controls its reaction speed by controlling (temperature/surface area/catalyst).
Definition
surface area.  By dissolving slowly over time, the capsule exposes a small amount of medicine for reaction each hour.
Term
By using a catalyst, you (increase/decrease/do not change) the enthalpy of reaction (ΔH).
Definition

do not change.  See the diagram below, comparing a catalyzed to a noncatalyzed reaction.

 

 

[image]

Term

The enthalpy of reaction (ΔH) in the chemical reaction below is

 

 

[image]

Definition
negative 15 kJ
Term
When performing stoichiometry calculations, the coefficients of a balanced equation are interpreted as (gram/mole) ratios.
Definition
mole ratios
Term

If 3 moles of HCl are consumed in the reaction below, how many moles of FeCl3 are produced?

 

___ HCl + ___ Fe2O3 → ___ FeCl3 + ___ H2O

 

Definition
1 mole FeCl3 will be produced
Term

Given the equation ___ H2O → ___ H2 + ___ O2,

how many moles of H2O would be required to produce 2.5 moles of O2?

Definition
5 moles H2O
Term

Consider the equation __ CaCO3 → __ CaO + __ CO2.

If 3 moles of calcium carbonate decomposes according to the reaction above, how many grams of CO2 are produced?

Definition
132 grams
Term

If 146 grams of HCl are are used in the reaction

___ HCl + ___ Fe2O3 → ___ FeCl3 + ___ H2O,

how many moles of FeCl3 are produced?

Definition
1.3 moles FeCl3
Term

In the reaction ___ Zn + ___ H2SO4 → ___ ZnSO4 + H2,

how many grams of H2SO4 are required to produce 1.0 gram of H2?

Definition
49 grams H2SO4
Term

Methane undergoes a combustion reaction to produce carbon dioxide and water vapor:

 

___ CH4 + ___ O2 → ___ CO2 + ___ H2O

 

If 6600 grams of CO2 are produced, what mass of oxygen gas was required?

Definition
9600 grams of O2 was required
Term

Given the reaction __ Zn + __ HCl → __ ZnCl2 + __ H2 ,

if 2 mol Zn and 5 mol HCl are allowed to react, what is the correct amount of ZnCl2 produced?

Definition

This is a limiting reactant problem, since amounts of both reactants are given to you.

 

By completing the stoichiometry, 2 mol Zn will produce 2 mol ZnCl2 and 5 mol HCl will produce 2.5 mol ZnCl2.  So the correct amount is the lower amount, 2 mol ZnCl2

Term
If amounts of both reactants are given to you in a stoichiometry problem, one of the reactants will be used up first, and we call that reactant the (excess/limiting) reactant.
Definition
limiting
Term
The starting amount of the (excess/limiting) reactant produces the correct amount of product in a chemical reaction.
Definition
limiting
Term
Can you draw out the stoichiometry roadmap?
Definition
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