Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
31 Cards in this Set
- Front
- Back
|
What is kinetic energy |
Energy in motion |
|
|
What is potential energy |
Energy stored in an object |
|
|
What is entalpy |
The total amount of energy in chemicals (heat content |
|
|
What Is the standard condition |
When all elements in there normal physical stage or standard condition at 298K and 101 Kpa has an enthalpy of 0 |
|
|
How come it is possible to measure enthalpy changes |
Because when heat energy is exchanged with the environment within a chemical reaction differences can be measured |
|
|
What is the symbol for enthalpy change |
^H delta |
|
|
What is the standard enthalpy change |
This is referred to a reaction done under standard conditions and with everyone present in the standard stage |
|
|
What must the concentration always equal too if u have a solution |
1 mol/dm3 |
|
|
What is the symbol for standard enthalpy change |
^H• (teta •) |
|
|
What is the formula for heat change ^H |
^H=^H• (products)-^H•(reactants) |
|
|
What is an endothermic reaction |
This is when heat is lost to the environment it causes an increase in temperature and becomes hot. The answer is always negative |
|
|
Why are decomposition reactions usually endothermic |
Because energy is required to break the bonds so is therefore absorbed |
|
|
What is an endothermic reaction |
This is when heat is absorbed from the environment. The temperature is decreased and the reaction becomes cooler. The answer is always positive |
|
|
Why are synthesis reactions always exothermic |
Because energy is released to make new bonds |
|
|
Represent the energy level diagram for exothermic reaction and explain which has the most energy (reactants/products |
Look in text |
|
|
Represent the energy level diagram for endothermic reaction and explain which has most energy (reactants/products |
Look in text |
|
|
What is the standard enthalpy change of reaction |
This is the heat change that occur when equal quantities of material react under standard conditions and with everything in each standard stage |
|
|
What is the symbol for standard enthalpy change of reaction |
^Hr |
|
|
What is the symbol for enthalpy change of formation. |
^Hf |
|
|
What is ^Hf |
This is the heat change which occurs when 1 mole of a compound is formed from its element under standard condition and with everything in its standard stage. |
|
|
What is the symbol for standard enthalpy change or combustion |
^Hc |
|
|
What is ^Hc |
This is the heat change when one mole of the compound is burned completely in oxygen under standard condition and everything in its standard stage |
|
|
What is the symbol for standard enthalpy change of hydration |
^Hhyd |
|
|
What is ^Hhyd |
This is the heat change when 1 mole of a specified gaseous ion dissolve in enough water to form an infinitely dilute solution under Standard condition |
|
|
What is lattice energy |
This is the enthalpy change when one mole of an ionic compound is formed from its gaseous ion under standard conditions. |
|
|
Is lattice energy always exothermic |
Yes |
|
|
What is standard enthalpy change of atomization |
This is the heat change when one mole of a gaseous atom is formed from an element in there standard and under standard conditions |
|
|
What is standard enthalpy change of atomization always endothermic |
Becyto change any state to a gaseous bonds needs to broken and therefore energy needs to be absorbed |
|
|
What is standard enthalpy change of neutralization |
This is the heat change when one mole of water is produced in a reaction between an acid and a base |
|
|
What is the standard enthalpy change of solution (^Hsol) |
This is the heat change when 1 mole of a substance is dissolved in a very large amount of water under standard conditions |
|
|
What is bond energy |
This is the amount of energy needed to break 1 mole of a gaseous bond in one mole of a gaseous molecule |
