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Problem 58b
Suppose you were dissatisfied with both Celsius and Fahrenheit units and wanted to design your own temperature scale based on ethyl alcohol (ethanol). On the Celsius scale, ethanol has a melting point of -117.3 °C and a boiling point of 78.5 °C, but on your new scale calibrated in units of degrees ethanol, °E, you define ethanol to melt at 0 °E and boil at 200 °E. (b) How does an ethanol degree compare in size with a Fahrenheit degree?
Problem 58c
Suppose you were dissatisfied with both Celsius and Fahrenheit units and wanted to design your own temperature scale based on ethyl alcohol (ethanol). On the Celsius scale, ethanol has a melting point of -117.3 °C and a boiling point of 78.5 °C, but on your new scale calibrated in units of degrees ethanol, °E, you define ethanol to melt at 0 °E and boil at 200 °E. (c) What are the melting and boiling points of water on the ethanol scale?
Problem 58d
Suppose you were dissatisfied with both Celsius and Fahrenheit units and wanted to design your own temperature scale based on ethyl alcohol (ethanol). On the Celsius scale, ethanol has a melting point of -117.3 °C and a boiling point of 78.5 °C, but on your new scale calibrated in units of degrees ethanol, °E, you define ethanol to melt at 0 °E and boil at 200 °E. (d) What is normal human body temperature (98.6 °F) on the ethanol scale?
Problem 58e
Suppose you were dissatisfied with both Celsius and Fahrenheit units and wanted to design your own temperature scale based on ethyl alcohol (ethanol). On the Celsius scale, ethanol has a melting point of -117.3 °C and a boiling point of 78.5 °C, but on your new scale calibrated in units of degrees ethanol, °E, you define ethanol to melt at 0 °E and boil at 200 °E. (e) If the outside thermometer reads 130 °E, how would you dress to go out?
- Sodium chloride has a melting point of 1074 K and a boil-ing point of 1686 K. Convert these temperatures to degrees Celsius and to degrees Fahrenheit.
Problem 60
- A 125 mL sample of water at 293.2 K was heated for 8 min, 25 s so as to give a constant temperature increase of 3.0 °F/min. What is the final temperature of the water in degrees Celsius?
Problem 61
- What is the difference between a derived SI unit and a funda-mental SI unit? Give an example of each
Problem 62
- What is the volume in L of a cube with an edge length of 7.0 dm?
Problem 64
- What is the volume in mL of a cube with an edge length of 2.5 cm?
Problem 65
- What is the density of glass in g/cm3 if a sample weighing 27.43 g has a volume of 12.40 cm3?
Problem 66
- What is the density of lead in g/cm3 if a sample weighing 206.77 g has a volume of 15.50 cm3?
Problem 67
- A vessel contains 4.67 L of bromine whose density is 3.10 g/cm3. What is the mass of the bromine in the vessel (in kilograms)?
Problem 68
- Aspirin has a density of 1.40 g/cm3. What is the volume in cubic centimeters of an aspirin tablet weighing 250 mg? Of a tablet weighing 500 lb?
Problem 69
- Gaseous hydrogen has a density of 0.0899 g/L at 0 °C, and gaseous chlorine has a density of 3.214 g/L at the same tem-perature. How many liters of each would you need if you wanted 1.0078 g of hydrogen and 35.45 g of chlorine?
Problem 70
- The density of silver is 10.5 g/cm3. What is the mass (in kilo-grams) of a cube of silver that measures 0.62 m on each side?
Problem 71
- What is the density of lead in g/cm3 if a rectangular bar mea-suring 0.50 cm in height, 1.55 cm in width, and 25.00 cm in length has a mass of 220.9 g?
Problem 72
- What is the density of lithium metal in g/cm3 if a cylindrical wire with a diameter of 2.40 mm and a length of 15.0 cm has a mass of 0.3624 g?
Problem 73
- You would like to determine if a set of antique silverware is pure silver. The mass of a small fork was measured on a balance and found to be 80.56 g. The volume was found by dropping the fork into a graduated cylinder initially contain-ing 10.0 mL of water. The volume after the fork was added was 15.90 mL. Calculate the density of the fork. If the den-sity of pure silver at the same temperature is 10.5 g/cm3, is the fork pure silver?
Problem 74
- Label the following properties as intensive or extensive: den-sity, volume, mass, electrical conductivity.
Problem 75
- The density of chloroform, a widely used organic solvent, is 1.4832 g/mL at 20 °C. How many milliliters would you use if you wanted 112.5 g of chloroform?
Problem 76
- More sulfuric acid (density = 1.8302 g/cm3) is produced than any other chemical—approximately 3.6 * 1011 lb/yr world-wide. What is the volume of this amount in liters?
Problem 77
Problem 78
Which has more kinetic energy, a 1400 kg car moving at 115 km/h or a 12,000 kg truck moving at 38 km/h?
Problem 79
Assume that the kinetic energy of a 1400 kg car moving at 115 km/h (Problem 1.78) is converted entirely into heat. How many calories of heat are released, and what amount of water in liters could be heated from 20.0 °C to 50.0 °C by the car's energy? (One calorie raises the temperature of 1 mL of water by 1 °C)
- Sodium (Na) metal undergoes a chemical reaction with chlorine (Cl) gas to yield sodium chloride, or common table salt. If 1.00 g of sodium reacts with 1.54 g of chlorine, 2.54 g of sodium chloride is formed and 17.9 kJ of heat is released, how much sodium and how much chlorine in grams would have to react to release 171 kcal of heat?
Problem 81
- A Big Mac hamburger from McDonald’s contains 540 Calories. (a) How many kilojoules does a Big Mac contain?
Problem 82
- A 20 fluid oz. soda contains 238 Calories. (a) How many kilojoules does the soda contain? (b) For how many hours could the amount of energy in the soda light a 75-watt light bulb? (1 watt = 1 J/s)
Problem 83
- Which of the following statements uses exact numbers? (a) 1 ft = 12 in. (b) 1 cal = 4.184 J (c) The height of Mt. Everest is 29,035 ft. (d) The world record for the 1-mile run, set by Morocco's Hicham el Guerrouj in July 1999, is 3 minutes, 43.13 seconds
Problem 84
- What is the difference in mass between a nickel that weighs 4.8 g and a nickel that weighs 4.8673 g?
Problem 85
Problem 86a
How many significant figures are in each of the following measurements? (a) 35.0445 g
Problem 86b
How many significant figures are in each of the following measurements? (b) 59.0001 cm