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Chem Final Unit 4
This will contain important info from Unit 4
Question | |
---|---|
What is the first law of Thermodynamics? | Nrg can flow in or out of a system through heat and work or a system can gain nrg through surroundings and vice versa. |
What is important about energy? | It can neither be created nor destroyed, just transferred from one place to another |
What is an open system? | A system where matter can enter and exit |
What is a closed system? | A system where matter cannot enter but nrg (heat) can |
What is an isolated system? | A system where matter and nrg cannot enter or leave (fixed) |
What is the internal nrg equation? | delta E = q + w |
What happens when work is negative? | Means work is done by system |
What happens when work is positive? | Means work is done on system |
What happens when q (heat) is positive? | The system is absorbing nrg -- endothermic |
What happens when q (heat) us negative? | The system is releasing nrg -- exothermic |
What is the 2nd law of Thermodynamics? | Heat naturally flows from hot to cold (spontaneous) having the entropy increase |
What is important about heat in the 2nd law of Thermodynamics? | Heat doesn't naturally flow from cold to hot |
What is q measured in? | Joules or cal |
What is the equation for work? | w = -P deltaV |
What is the equation for heat? | q = mc deltaT |
What does q = mc deltaT calculate? | Calculates the amount of heat absorbed or released whenever there is a temperature change |
What is the latent heat of fusion and vaporization. | q = deltaH fus q = deltaH vap |
What do the equations of latent heat of fusion and vaporization mean? | Calculate the amount of heat absorbed or released whenever there is a phase change |
If you are given a calorimeter cup, what is it and what is it used for? | A calorimeter Used for finding changes in temps |
What is a system? | whatever you are investigating or examining |
What are surroundings? | whatever is coming in contact with that system |
What is the calorimetry equation? | -q metal = q water |
A 32.5 g sample o copper at 45.8 degrees Celsius is placed into 105.3g of water at 15.4 degrees Celsius. What is the final temperature? specific heat of copper = 0.385 J/g C specific heat of water = 4.18 J/g C | Tf = 17.2 degrees celsius |