6950920
Description
Flashcards by Leisey Kennedy, updated more than 1 year ago
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Created by Leisey Kennedy
about 8 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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