e temperature of an object increases by 43.3 °C when it absorbs 3851 J of heat. Calculate the heat capacity of the object. = e mass of the object is 371 g. Use the table of specific heat values to identify the composition of the object. Substance gold Specific heat (J/(g · °C)) . 0.129 silver 0.240 iron 0.444 aluminum 0.900 The object is composed of 000 О gold. aluminum. silver. iron. J/°

e temperature of an object increases by 43.3 °C when it absorbs 3851 J of heat. Calculate the heat capacity of the object. = e mass of the object is 371 g. Use the table of specific heat values to identify the composition of the object. Substance gold Specific heat (J/(g · °C)) . 0.129 silver 0.240 iron 0.444 aluminum 0.900 The object is composed of 000 О gold. aluminum. silver. iron. J/°

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 9.13-g sample of vanadium is heated to 99.10 °C and is then placed into 20.0 g water in a calorimeter. The water temperature rises from 20.51 to 24.46 °C. Calculate the specific heat of vanadium.
A 350.0 g iron pot is heated on a stove for a period of time until it is hot. The stove is turned off and 516 g of cold water (10.0 °C) is added to the pot. When thermal equilibrium is reached, the temperature of the water is 28.4 ° C. What was the initial temperature of the iron pot, assuming heat was exchanged between these two objects and none was lost to the surroundings? (The specific heat capacity of iron is 0.450 J/g °C. The specific heat capacity of water is 4.184 J/g °C) Give only the numerical answer in the box and not units. Give 4 sig figs in your answer. Show the calculations for the problem by writing it on a paper, upload the image file/pdf file in the question for file upload.
A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g * C.
33.79 g of a solid is heated to 100.°C and added to 50.0 g of water in a coffee cup calorimeter and the contents are allowed to sit until they finally have the same temperature. The water temperature changes from 29.76 °C to 38.3 °C and the specific heat capacity of water is 4.184J/g °C. What is the specific heat capacity (in J/g°C) of the solid? O 1.73 O 1.17 O 0.857 O 0.579
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
If 0.064 mol of hydrochloric acid (HCl) is mixed with 0.064 mol of sodium hydroxide (NaOH) in a "coffee cup" calorimeter, the temperature of 4.9 g of the resulting solution increases from 25.0°C to 30.0°C.Given that the energy released is 1.2 × 101 cal when the specific heat of the resulting solution is 1.00 cal/g−°C, use a conversion factor to convert the energy released to joules (J).
The temperature of an object increases by 43.5 °C when it absorbs 3829 J of heat. Calculate the heat capacity of the object. C = The mass of the object is 367 g. Use the table of specific heat values to identify the composition of the object. Substance Specific heat (J/(g. °C)) gold 0.129. silver 0.240 iron 0.444 aluminum 0.900 The object is composed of O aluminum. silver. gold. iron. J/°C
When 14.2 g KBr is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature drops from 28.88 °C to 23.38 °C. What is the enthalpy change per gram of KBr dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g·K.
A 135.0-g sample of a metal at 153.0 °C is added to 255.0 g of ethylene glycol (specific heat = 2.43 J/g･ °C) in a calorimeter at 25.7 °C. The temperature of the ethylene glycol rises to 38.2 °C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the ethylene glycol.
What mass of water will change its temperature by 10 °C when 975 J of heat is added? The specific heat of water is 4.18 J/g 0C
The specific heat of aluminum is 0.897 J/g·°C and the specific heat of water is 4.18 J/g·°C. If a 3.00 g piece of aluminum at 300.0°C is immersed in 10.0 mL of water at 30.0°C, predict the final temperature of the mixture.
A sample of aluminum, initially at 5.0 °C, was placed in 18.0 g of water, initially at 25.0 °C. The final temperature of the water and the metal was 21.0 °C. The specific heat of water is 4.184 J g-1 °c-1 and aluminum is 0.940 J g-1 °C-1. Ignore the heat capacity of the container. What is the mass (in g) of the aluminum?