Surrealism-The M. New folder G Genetic drift - Wikip lorris -Specific Heat Practice D O View Insert Format Tools Add-ons Help Accessibility Last edit 22 + BIUA 100% - Normal text New Rocker 8. A 53.0 gram nickel bolt (c = 0.44 J/g°C) is heated until it glows and is then dropped into 722 grams of water (originally at 25°C) After they reach equilibrium, they both have a temperature of 42°C. What was the high temperature of the bolt? %3D Note: 1 kilogram = 1000 grams 1 Calorie = 1 kcal = 1000 calories OF to °C: [(T-32 ) x 5 ]-9 9. A 65.5 gram piece of glass (c = 0.840 J/g°C) is heated to 177°C and dropped into a beaker containing 450 grams of ethanol (c = 2.46 J/g°C.) After they reach equilibrium, their temperature is 51.0°C. What was the starting temperature of the ethanol? lili

Surrealism-The M. New folder G Genetic drift - Wikip lorris -Specific Heat Practice D O View Insert Format Tools Add-ons Help Accessibility Last edit 22 + BIUA 100% - Normal text New Rocker 8. A 53.0 gram nickel bolt (c = 0.44 J/g°C) is heated until it glows and is then dropped into 722 grams of water (originally at 25°C) After they reach equilibrium, they both have a temperature of 42°C. What was the high temperature of the bolt? %3D Note: 1 kilogram = 1000 grams 1 Calorie = 1 kcal = 1000 calories OF to °C: [(T-32 ) x 5 ]-9 9. A 65.5 gram piece of glass (c = 0.840 J/g°C) is heated to 177°C and dropped into a beaker containing 450 grams of ethanol (c = 2.46 J/g°C.) After they reach equilibrium, their temperature is 51.0°C. What was the starting temperature of the ethanol? lili

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter10: Energy

Section: Chapter Questions

Problem 38QAP: In the “Chemistry in Focus” segment Firewalking: Magic or Science?, it is claimed that one reason...

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The complete combustion of acetylene, C2H2(g), produces 1300. kJ of energy per mole of acetylene consumed. How many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal water by 10.0c if the process is 80.0% efficient? Assume the density of water is 1.00 g/cm3
9.86 You make some iced tea by dropping 134 g of ice into 500.0 mL of warm tea in an insulated pitcher. If the tea is initially at 20.0°C and the ice cubes are initially at 0.0°C, how many grams of ice will still be present when the contents of the pitcher reach a final temperature? The tea is mostly water, so assume that it has the same density (1.0 g/mL), molar mass, heat capacity (75.3 J K-1 mol-1), and heat of fusion (6.0 kJ/mol) as pure water. The heat capacity of ice is 37.7 J K-l mol-l.
A 500-g sample of one of the substances listed in Table 7-1 was heated from 25.2C to 55.1C, requiring 133 J to do so. Which substance was it?
Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
9.100 Two baking sheets are made of different metals. You purchase both and bake a dozen cookies on each sheet at the same time in your oven. You observe that after 9 minutes, the cookies on one sheet are slightly burned on the bottom, whereas those on the other sheet are fine. (You are curious and you vary the conditions so you know the result is not caused by the oven.) (a) How can you use this observation to infer something about the specific heat of the materials in the baking sheets? (b) What is themathematical reasoning (equation) that you need to support your conclusion?
9.102 A runner generates 418 kJ of energy per kilometer from the cellular oxidation of food. The runner's body must dissipate this heat or the body will overheat. Suppose that sweat evaporation is the only important cooling mechanism. If you estimate the enthalpy of evaporation of water as 44 kJ/mol and assume that sweat can he treated as water, describe how you would estimate the volume of sweat that would have to be evaporated if the runner runs a 10-km race.
The addition of 3.15 g of Ba(OH)28H2O to a solution of 1.52 g of NH4SCN in loo g of water in a calorimeter caused the temperature to fall by 3.1 C. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)28H2O(s)+2NH4SCN(aq)Ba(SCN)2(aq)+2NH3(aq)+10H2O(l)
A cubic piece of uranium metal (specific heat capacity = 0.117 J/C g) at 200.0C is dropped into 1.00 L deuterium oxide ("heavy water;" specific heat capacity = 4.21 I J/C g) at 25.5C. The final temperature of the uranium and deuterium oxide mixture is 28.5C. Given the densities of uranium (19.05 g/cm3) and deuterium oxide (1.11 g/mL). what is the edge length of the cube of uranium?
In the “Chemistry in Focus” segment Firewalking: Magic or Science?, it is claimed that one reason people can walk on hot coals is that human tissue is mainly composed of water. Because of this, a large amount of heat must be transferred from the coals to change the temperature of the feet significantly. How much heat must be transferred to 100.0 g of water to change its temperature by 35 °C?
When calcium carbonate, CaCO3 (the major constituent of limestone and seashells), is heated, it decomposes to calcium oxide (quicklime). CaCO3(s)CaO(s)+CO2(g);H=177.9kJ How much heat is required to decompose 21.3 g of calcium carbonate?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.