A18 kg block of iron at 29 °C is rapidly heated by a torch such that 11 kJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (11 kJ ) was quickly transferred to a 860 g pellet of copper at 22°C, what temperature would the copper reach before it begins losing heat to the surroundings? Use the equation for heat capacity and the following heat capacity values: mc, AT %3D 0.450 J/(g C) 0.385 J/(g C) Cs, Fe(s) Cs, Cu(s) Express the final temperatures of the iron and copper in C to two significant figures separated by a comma.

A18 kg block of iron at 29 °C is rapidly heated by a torch such that 11 kJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (11 kJ ) was quickly transferred to a 860 g pellet of copper at 22°C, what temperature would the copper reach before it begins losing heat to the surroundings? Use the equation for heat capacity and the following heat capacity values: mc, AT %3D 0.450 J/(g C) 0.385 J/(g C) Cs, Fe(s) Cs, Cu(s) Express the final temperatures of the iron and copper in C to two significant figures separated by a comma.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.82PAE: 9.82 The specific heat of gold is 0.13 J g-1 K-1 and that of copper is 0.39 J g-1 K-1. Suppose that...

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9.30 For the example of shallow water and sandy beaches, which material has a larger heat capacity or specific heat? How does a hot day at the beach provide evidence for your answer?
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
9.32 The material typically used to heat metal radiators is water. If a boiler generates water at 79.5°C, what mass of water was needed to provide the heat required in the previous problem? Water has a specific heat of 4.184Jg1 C1 .
Consider the following specific heats of metals. Metal Specific Heat copper 0.385 J/(gC) magnesium 1.02 J/(gC) Mercury 0.138 J/(gC) Silver 0.237 J/(gC) Four 25-g samples, one of each metal, and four insulated containers with identical water volumes, all start out at room temperature. Now suppose you add exactly the same quantity of heat to each metal sample. Then you place the hot metal samples in different containers of water (that all have the same volume of water). Which of the answers below is true? a The water with the copper will be the hottest. b The water with the magnesium will be the hottest. c The water with the mercury will be the hottest. d The water with the silver will be the hottest. e The temperature of the water will be the same in all the cups.
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?
9.31 A metal radiator is made from 26.0 kg of iron. The specific heat of iron is 0.449Jg1C1 . How much heat must be supplied to the radiator to raise its temperature from 25.0 to 5 5.0°C?
Consider the following reaction in the vessel described in Question 57. A(g)+B(g)C(s)For this reaction, E=286 J, the piston moves up and the system absorbs 388 J of heat from its surroundings. (a) Is work done by the system? (b) How much work?
In the process of isolating iron from its ores, carbon monoxide reacts with iron(III) oxide, as described by the following equation: Fe2O3(s)+3CO(g)2Fe(s)+3CO2(g)H=24.8kJ The enthalpy change for the combustion of carbon monoxide is 2CO(g)+O2(g)2CO2(g)H=566kJ Use this information to calculate the enthalpy change for the equation 4Fe(s)+3O2(g)2Fe2O3(s)H=?
9.82 The specific heat of gold is 0.13 J g-1 K-1 and that of copper is 0.39 J g-1 K-1. Suppose that we heat both a 25-g sample of gold and a 25-g sample of copper to 80C and then drop them into identical beakers containing 100 mL of cold water at 10°C. When each beaker reaches thermal equilibrium, which of the following will be true, and why? (You should not need to calculate the actual temperatures here.) (a) Both beakers will be at the same temperature. (b) The beaker with the copper sample in it will be at a higher temperature. (c) The beaker with the gold sample in it will be at a higher temperature
What mass of carbon monoxide must be burned to produce 175 kJ of heat under standard state conditions?
A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5 C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.7 C. When thermal equilibrium is reached, the final temperature is 24.3 C. Calculate the specific heat capacity of titanium.
A block of aluminum and a block of iron, both having the same mass, are removed from a freezer and placed outside on a warm day. When the same quantity of heat has flowed into each block, which block will be warmer? Assume that neither block has yet reached the outside temperature. (See Table 6.1 for the specific heats of the metals.)

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