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27 Nov 2019

1. A 88.3 g sample of metal at 95.24 ^oCis added to 35.10 g of water that is initially at 17.27^oC.The final temperature of both the water and the metal is29.20^oC.The specific heat of water is 4.184 J/(g^oC).Calculate the specific heat of the metal.

2. A 56.4 g sample of Al at 93.3 ^oCis added to 173.7 g of water that is initially at 27.0^oC.The specific heat of Al and water are 0.90 J/(g^oC)and 4.184 J/(g^oC),respectively. Calculate the equilibrium temperature.

A 66 mL solution of a dilute AgNO₃solution is added to 88 mL of a base solution in a coffee-cupcalorimeter. As AgOH (s) precipitates, the temperature of thesolution increases from 23.35 ^oCto 25.65 ^oC.Assuming the mixture has the same specific heat(4.184J/g^oC)and density (1.00 g/cm³or 1.00 g/mL)as water, calculate the heat (in J) transferred to thesurroundings, q_surr.

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Elin HesselLv2

21 Jun 2019

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A 103 mL solution of a dilute acid is added to 106 mL of a basesolution in a coffee-cup calorimeter. The temperature of thesolution increases from 23.05 oC to 28.48 oC. Assuming the mixturehas the same specific heat (4.184J/goC) and density (1.00 g/cm3) aswater, calculate the heat (in J) transferred to the surroundings,qsurr.

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For a particular reaction, DeltaH = -111.4 kJ and DeltaS = -25.0 J/K. Calculate DeltaG for this reaction at 298 K Classify the following phase changes by the signs of the system's DeltaH and DeltaS. Consider these reactions, where M represents a generic metal. Use the information above to determine the enthalpy of the following reaction. Consider these reactions, where M represents a generic metal. 2M(s) + 6HCl(aq) rightarrow 2MCl3(aq) + 3H2(s) Delta H1, = -650.0 kJ HCl(g) rightarrow HCI(aq) Delta H2 = -74.8 kJ H2(g)+Cl2(g) rightarrow 2HC1(g) Delta H3 = -1845.0kJ MCI3(S) rightarrow MCI3(aq) Delta H4 = -416.0kJ Use the information above to determine the enthalpy of the following reaction 2M(S) + 3CI2(g) rightarrow 2MCI3(S) Delta H = A researcher studying the nutritional value of a new candy places a 4.20-gram sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.17 degree C. If the heat capacity of the calorimeter is 34.00 kJ K-1, how many nutritional Calories are there per gram of the candy? When 1.250 x 103 J of heat energy is added to 43.5 g of hexane, C6H14, the temperature increases by 12.7 degree C. Calculate the molar heat capacity of C6H14. If you have 420.0 mL of water at 25.00 degree C and add 130.0 mL of water at 95.00 degree C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water. A 54.21 g sample of a substance is initially at 24.2 degree C. After absorbing 2755 J of heat, the temperature of the substance is 108.6 degreeC. What is the specific heat (c) of the substance? If a system has 325 kcal of work done to it, and releases 5.00 times 102 kJ of heat into its surroundings, what is the change in internal energy of the system? Classify each of the following as a path function or a state function. A 1687 kg car is traveling down the road at 105.0 km/h. While traveling at this rate of speed, what is the kinetic energy of this vehicle in kilojoules? Convert the following energy units, 451 kJ to J 2060 kcal to kJ 9.77 x 106 J to kcal

1.A block of metal has dimensions 5.00 cm x 2.50 cm x 3.00 cm. Calculate the volume of the block, showing the answer to the correct number of significant figures and unit.

2.If the block of metal from question 2 has a mass of 405.3 g, what is the density of the metal? Calculate the density, showing the answer to the correct number of significant figures and correct unit.

3.Convert the numerical value of the density in question 2 from units of grams per cubic centimeter (g / cm3) to milligrams per milliliter (mg / mL). Note:

-there are 1000 milligrams in a gram.

-the volume unit cubic centimeter cm3 equals the milliliter mL.

Keep the new density to the same significant figures as you reported in question 2

4.A finely-powdered white solid is known to be homogeneous mixture rather than a pure substance. A sample of this solid completely dissolves in water. Give TWO possible substances that could make up this solid mixture, and briefly explain your choices.

5.If your percent SALT in Lab 2 is relatively low, it can be assumed that some salt did not go into the filtrate (the liquid that passes through the filter paper), but rather may have been trapped with the sand. Explain briefly how you could recover any of this "missing" salt?

6.A brand of aspirin claims to contain 325 mg (1 g = 1000 mg) of aspirin per tablet. In addition to pure aspirin, a tablet also contains a non-active filler. We assume that the tablet contains only these two components: aspirin and filler. If a single tablet weighs 1.17 g, calculate the percent filler. Hint: calculate percent aspirin FIRST using the formula

% aspirin = [ (mass aspirin Ã· mass tablet) x 100], the find % filler. When using this formula, make sure the masses of aspirin and tablet have the same units.

7.Water has a density of 1.00 g/mL, and chloroform has a density of 1.49 g/mL. These two liquids do not mix with each other, but rather, form two layers when combined.

8.Equal volumes of water and chloroform are placed in a beaker. A piece of nylon is dropped in the beaker, and is seen to float the the interface (the boundary) of the two liquid layers.

Give a possible value for the density of nylon, including the correct units. Explain your answer briefly.

9.A procedure similar to that used in Lab 3 was performed to find the density of cyclohexane, which has an actual density of 0.779 g/mL, Due to poor lab technique, an experimental density of only 0.663 g/mL is found. Calculate the percent error for the density. Give your answer to the correct number of significant figures.

10.Two white powders are given to you. One is pure sodium bicarbonate, and the other is baking powder (a mixture of sodium bicarbonate and a weak acid like citric acid). Which single test (NOT counting the visual examination with a hand lens) used in Lab 3 allows you to distinguish sodium bicarbonate from baking powder? Explain your answers completely.

11.Gold has a specific heat of 0.129 J/g^oC. If a piece of gold (initially at 10.0^oC) is dropped into hot water, the final temperature of both the gold and the water is measured as 70.9^oC. If it is known that 4560 J of heat transferred from the hot water to the gold, what is the mass of the piece of gold in grams? Give your answer to the correct number of significant figures.

12.It is stated in the Introduction to Lab 4 that q_water = -q_metal. This equation means that if a hot piece of metal is placed in water, the amount of heat given off by the metal is exactly equal to the amount of heat absorbed by the water. However, this equation is not always accurate, because not all of the heat from the metal necessarily goes to the water. Where else can some of the heat go if it is not absorbed by the water?

13.A certain brand of breakfast cereal claims to have 100 Calories per 28 gram serving. 150.0 grams of cereal are burned using a procedure similar to that used in Lab 4. How many calories of heat are released? Note 1 food Calorie (capital C) = 1000 heat calories (lower case c)

14.The oxalate anion C2O42- is found in many dark green vegetables, including spinach, swiss chard, and collard greens. When cations react with oxalate, the resulting ionic compounds are insoluble in water except Group I A oxalates (e.g. compounds of lithium, sodium, potassium, etc. and oxalate) and ammonium oxalate (NH4)2C2O4. These exceptions are soluble in water.

15.Spinach leaves are cut into small pieces, mashed with small amounts of boiling water, and filtered through filter paper to remove the insoluble spinach material. The resulting aqueous extract contains the oxalate anion.if a small amount of the spinach extract is mixed with a small amount of a calcium acetate solution, Ca(C2H3O2)2(aq), what do you expect will be observed?

16.If a small amount of the spinach extract from question 16 is mixed with a small amount of a potassium acetate solution, KC₂H₃O₂(aq), what do you expect will be observed?

17.If a hot water extract of another vegetable is mixed with calcium acetate solution and a white precipitate is observed, does this automatically indicate the presence of the oxalate anion in this vegetable? Explain your answer.

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