Term 4 chemistry exam

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Revision cards for 2016 Term 4 Chemistry
Leisey Kennedy
Flashcards by Leisey Kennedy, updated more than 1 year ago
Leisey Kennedy
Created by Leisey Kennedy over 7 years ago
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Question Answer
Gas pressure Gas particles colliding with walls of container. Atmospheric pressure measured with barometer. SI unit: pascal (Pa) other units: mm Hg, atm
Converting pressure units 1atm=760mm Hg= 101.3 kPa (kPa is 1000 Pa) kPa --> atm: divide by 101.3 atm --> kPa: multiple by 101.3 mm Hg --> atm: divide by 760 atm --> mm Hg: multiply by 760
Boyles Law Increasing pressure on gas will decrease volume P1V1=P2V2 (only applies to an ideal gas)
Ideal gas a hypothetical gas whose molecules occupy negligible space and have no interactions, and which consequently obeys the gas laws exactly. will not liquidate follow kinetic theory
Charles's Law changing the temperature changes the volume occupied. low temp = low volume high temp= larger volume Temp must be in Kelvin V1/T1=V2/T2
Kelvin C--> K 0 degrees C = 273K
Gay-Lussac's Law: Pressure and Temperature If volume is constant, as temperature increases, pressure increases. Temp is in K P1/T1=P2/T2
The combined gas law Calculations when the amount (moles) of gas is constant P1V1/T1=P2V2/T2
Real Gases Real gases will not follow gas laws at high pressures or low temps because size of gas particles becomes important. Particles become closer and take up more space.
Volume of gases STP is 0 degrees and 0 atm. At STP 1 mol = 22.4L Volume of gas = number of moles x 22.4
Properties of Gas 1. low density 2. spread 3. Exert pressure all directions 4. diffuse easily and quickly 5. Easily compressed
Kinetic Molecular Theory 1. Gases made of particles moving rapid and constant 2. Higher temp, faster move. (increased kinetic energy) 3. forces of attraction and repulsion between particles practically 0 4. Particles far apart. Volume of particles is small compared to volume occupied 5. Particles collision is elastic. No kinetic energy lost.
Enthalpy Enthalpy (H) is the heat content of a system. Change in enthalpy Δ (change in) H is given by: ΔH=H(products)- H(reactants)
Exothermic reactions heat is release into surroundings ΔH is negative feels hot
Endothermic Reactions heat is absorbed from the surroundings Δ H is positive feels cold
Dalton's Law The total pressure in a gas mixture is the sum of the particle pressures of each individual gas. P total = P1+P2+P3+...
Le Chatelier's Principle If a change is applied to a system at equilibrium, system system reacts to counteract change and return to equilibrium.
Changing temperature In exothermic reaction, if heated (product) reaction is pushed to left. In endothermic reaction, if heated (reactant) reaction is shifted to right. Decreasing has reverse effect.
Changing pressure Increasing pressure favours side with less particles Decreasing pressure favours side with more particles
Chemical Equilibrium When the rates of the forward and reverse reactions are equal, a state of balance has been reached.
Changing concentration Product increases - shifts to right side Product reduces- shifts back to the left
Breathing and respiration C6H12O6(s) + 6O2(g) --> 6CO2(g)+ 6H2O(g) ΔH= -2803 kj/m
pH calculation pH of 0.05M solution of hydrochloric acid: [H+] = 0.05M pH=-log10[H+] =-log(0.05) =-(-1.3) =1.3
Neutralisation Reactions acid and base react in aqueous solution produce salt and water. Eg: HCl + NaOH --> NaCl + H2O acid base salt water
Logs
Example Neutralisation Reaction Question How many moles of sulphuric acid are required to neutralize 0.5mol of sodium hydroxide? H2SO4 + 2NaOH --> Na2SO4 + 2H2O Use mole ratio:
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