inter and intra molecular forces
Moles
Conservation of Matter
Gas and Solutions
Thermochemistry
100
What is the strongest intermolecular force?
Hydrogen bonding
100
What is Avogadro's number?
6.02 x 1023
100
What does the law of conservation of mass state?
Mass in neither created or destroyed: what goes in must come out!
100
atm stands for?
Atmosphere
100
When your body is warmed by an electric blanket during the winter, is this process endothermic or exothermic?
Endothermic
200
What is the weakest intermolecular force?
London Dispersion Force
200
How many molecules are in 1 mole of NO2?
6.02 x 1023 molecules
200
Are Reactants on the left or the right side of the arrow in a chemical equation?
Left
200
What unit for temperature is required for calculating gas laws: Celsius, Kelvin, Fahrenheit, or Suns?
Kelvin
200
The enthalpy of a system is the same as the _____?
heat content
300
Which of the following has the highest boiling point, H2 or NH3?
NH3
300
What is the molar mass of Oxygen?
16 g/mol
300
How many oxygens are in the following reactants:
2H2O + NaPO4
6 oxygens
300
What is the units of molarity?
mole/Liter
300
2 Mg+ O2 --> 2MgO + 72.3 kJ
How much heat is involved in the production of 2 moles of MgO?
72.3 kJ
400
Substances with stronger intermolecular forces have ______boiling points that those with weaker forces.
higher
400
What do a mole and a dozen have in common?
Both are units used to count a number of items.
400
What is stoichiometry?
The relationship between the amounts of reactants and products of a chemical reaction.
400
In the following alloy, define the solvent: 75% Copper and 25% Nickel.
Copper
400
The SI unit of energy is?
Joule
500
Draw a hydrogen bond between H2O molecules.
500
What is the molar mass of H2?
2 g/mol
500
Is this chemical equation balanced?
C6H6 + 6H2 → C6H12
NO! 18 H on left and 12 H on the right!
500
What equation would you use to solve a dilution problem?
C1V1 = C2V2
500
What information can be obtained from a heating curve (just name 1)?
- Phase Transitions: The points where a substance transitions between solid, liquid, and gas phases (e.g., melting point and boiling point).
- Temperature Changes: The temperature range during each phase of the substance (solid, liquid, gas).
- Energy Changes: The amount of energy absorbed or released during heating or phase transitions.
- Plateaus: Flat sections on the curve that indicate phase changes where the temperature remains constant as energy is used to break intermolecular bonds (e.g., during melting or boiling).
- Specific Heat: The slope of the curve during temperature increases within a single phase reveals the specific heat of the substance in that phase.
- Latent Heat: The energy associated with phase changes, such as the heat of fusion (melting) or the heat of vaporization (boiling).