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Chemistry I Exam 4
| Question | Answer |
|---|---|
| Endothermic Reactions: | Heat will be absorbed into system; Surroundings will be cold; Positive Enthalpy |
| Exothermic Reactions: | Heat is released into system; Surroundings will be hot; Negative Enthalpy |
| Law of Conservation of Energy | Energy cannot be destroyed or created |
| Cooling: | the removal of energy (heat) |
| How will heat move? | Heat only moves from where there is a lot of heat (hot) to where there is a little of heat (cold). |
| " - " Enthalpy | - Enthalpy does not mean "negative energy"; It means that energy is leaving or being transferred out of it. |
| Energy Transferred Formula | q = (mass) (heat capacity) (∆T) |
| Heat Capacity of Water | 4.184 J/(g)(°C) |
| What happens if a reactant has a high heat capacity? | It will not be easily heated; It will be able to absorb a lot of energy; It will require the a high amount of energy to raise its temperature by 1 °C |
| How to find thermochemical ratios? | Use the mole - energy ratios to create them. |
| Hess's Law | Using multiple thermochemical equations to find the amount of energy required for a specific reaction; You must make sure that after canceling out, you are left with only the reactants of the specific reaction. |
| Standard Enthalpy of Formation | This is the natural state of the elements (Ex: O2 (g) ; H2 (g) ; F2; S8 (s) ; P4 (s); Ca (s) |
| Using Standard Molar Enthalpy of Formation | Reactants with just singular elements will have 0 kJ; (Sum of Products kJ) - (Sum of Reactants kJ) = ∆H |
| Using Bond Energy's | (Bond Energies of Reactants) - (Bond Energies of Products) = ∆H Must be the bond energies of the SPECIFIC type of bond (single, double, triple) |
| What's Internal Energy (∆E) of system? | Kinetic Energy + Potential Energy |
| Formula of Internal Energy, Heat, and Work | ∆E = q + w |
| Ideal Gas Equation | PV = nRT P = pressure (atm) V = volume (L) n = mass/molar mass (m/mm) R = gas constant (0.0820574 atm L/mol K) T = temperature (K) |
| K to Celsius | 0 ºC + 273.15 K |
| atm Conversions | 760 mm Hg; 760 torr |
| Pressure Formula | P final = P reactant + P reactant |
| Raising the Temperature of Gas at a Constant Volume: | The pressure of the gas will increase |
| Adding More Molecules to Sample at Constant Temperature and Volume: | The pressure of the gas will increase |
| If a gas molecule is Heavier? | It will move slower because it is heavier. |
| Effusion: | Movement of molecules through a small hole in a membrane into a vacuum without collisions |
| Grahams' Law | (r1/r2) = √(m2/m1) |
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