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Review Questions

# Review Questions - calculate results in the experiments 5...

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Review Questions: 1. What information can you determine using a calorimeter? You can determine the calorimeter heat capacity which also contributes to finding heat of fusion of ice and the specific heats of metals. 2. If two objects with differing heat capacities and temperatures are placed together, will the object with greater or lesser heat capacity have the largest change in the temperature? The lesser heat capacity will have the largest change in the temperature. 3. For a given process, where is heat flowing (which direction)? For example: adding cold to hot water, adding hot metal to cold water, adding cold metal to hot water, etc. In an endothermic reaction, heat is being flowed into the system, for an exothermic reaction, heat is being flowed out of the system and into the surroundings, 4. Why was the calorimeter calibrated? By calibrating the calorimeter we were able to calculate heat of fusions of ice, specific heats of metals, and heats of chemical reactions. The calibrated calorimeter helped
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Unformatted text preview: calculate results in the experiments. 5. The heat capacity of water is 1 cal/g˚C. How much energy is needed to increase the temperature of a gram of water 1˚C? How much energy is needed to heat 100g of water by 100˚C? 4.18 J/1 cal; 100 cal/g˚C 6. Solvation of an acid heats water up; for example, HCL(l) + H20(l) H+(aq) + CL-(aq) Do the products or reactants have more enthalpy? To where did the energy from the reaction flow? Reactants have more enthalpy and the energy flowed into the surroundings. 7. What does a negative q and positive q mean in calorimetry? Negative change of enthalpy which means an exothermic reaction and a positive change of enthalpy means that an endothermic reaction occurred. 8. If you put 25g of a substance at 25˚C into a calorimeter with 85g of the same substance at 85˚C, what is the final temperature of the mixture if the calorimeter has zero heat capacity? 60˚C is the final temperature of the mixture if the calorimeter has a zero heat capacity....
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