A 4.70-g sample of aluminum pellets (specific heat capacity = 0.89 J °C- g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J °C- g) are heated to 115.0°C. The mixture of hot iron and aluminum is then dropped into 98.3 g of water at 22.0°C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings. The specific heat capacity of water is 4.18 J °C¯'g¬! °C

A 4.70-g sample of aluminum pellets (specific heat capacity = 0.89 J °C- g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J °C- g) are heated to 115.0°C. The mixture of hot iron and aluminum is then dropped into 98.3 g of water at 22.0°C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings. The specific heat capacity of water is 4.18 J °C¯'g¬! °C

Chemistry

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Chapter6: Thermochemistry

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Problem 61E: A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of...

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A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J/C g) are heated to 100.0C. The mixture of hot iron and aluminum is then dropped into 97.3 g water at 22.0C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
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.
Alloys When a 58.8-g piece of hot alloy is placed in125 g of cold water in a calorimeter, the temperature ofthe alloy decreases by 106.1°C, while the temperature ofthe water increases by 10.5°C. What is the specific heat ofthe alloy?
You wish to heat water to make coffee. How much heat (in joules) must be used to raise the temperature of 0.180 kg of tap water (enough for one cup of coffee) from 30C to 96C (near the ideal brewing temperature)? Assume the specific heat is that of pure water, 4.18 J/(gC).
The specific heat capacity of copper is 0.385 J g1 C1, whereas it is 0.128 J g1 C1 for gold. Assume you place 100. g of each metal, originally at 25 C, in a boiling water bath at 100 C. If energy is transferred to each metal at the same rate, determine which piece of metal will reach 100 C first.
A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?
When a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 C to 26.9 C. The heat capacity of the calorimeter is 534 J/C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?
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)
Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures. A mixture of 2.00 mol of powdered aluminum and 3.00 mol of ammonium nitrate crystals reacts exothermically yielding nitrogen gas, water vapor, and aluminum oxide. How many grams of the mixture are required to provide 245 kJ of heat? See Appendix C for data.
How much will the temperature of a cup (180 g) of coffee at 95 C be reduced when a 45 g silver spoon (specific heat 0.24 J/g C) at 25 C is placed in the coffee and the two are allowed to reach the same temperature? Assume that the coffee has the same density and specific heat as water.
A 500.0-g sample of an element at 195C is dropped into an ice--water mixture; 109.5 g ice melts and an ice--water mixture remains. Calculate the specific heat of the element. See Exercise 131 for pertinent information.
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?

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