Review | Constants | Periodic TableThe molar heat capacity of silver is 25.35 J/mol - °C. How much energy would it take toraise the temperature of 9.20 g of silver by 20.0 °C?apacity,Express your answer with the appropriate units.View Available Hint(s)ergy requiredce by exactlyd to warm anobjectay life. Formore energymall cup.q =ValueUnitscities areunt of thed is to reporte temperaturey 1 degreeсaрacity,heat capacityA secondy it takes tofa substancelue is thethe symbol Cs.°C). The heatrelated to therature by an, where ne substance, orhe number ofSubmitPart CWhat is the specific heat of silver?Express your answer with the appropriate units.• View Available Hint(s)HAValueUnits

Part B : We would calculate heat required by using formula : q = n × Cm × ∆T Where, n = moles Cm…

Answered: The molar heat capacity of silver is…

The molar heat capacity of silver is 25.35 J/mol - °C. How much energy would it take to raise the temperature of 9.20 g of silver by 20.0 °C? Express your answer with the appropriate units.

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 calorimeter contained 79.0 g of water at 15.91°C. A 105-g sample of iron at 65.26°C was placed in it, giving a final temperature of 18.88°C for the system. Calculate the heat capacity of the calorimeter. Specific heats are 4.184 J/g-°C for H2O and 0.444 J/g-°C for Fe. Heat capacity of the calorimeter =| J/°C
A 1.75 g sample of zinc metal is reacted with 128 g of 1.10 M hydrochloric acid solution in a constant-pressure calorimeter. The resulting solution changes in temperature from 22.58 °C to 22.97 °C. The hydrochloric acid is in excess. Based on this information, and estimating the solution's heat capacity as 4.18 Jg1 °C, what is the amount of heat, in joules, transferred in this reaction?
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
calculate the heat (in J) of the reaction if 50.0 mL of HCl is added to 50.0 mL of NaOH in a coffee-cup calorimeter. The initial temperature for both solutions is 23.2oC. At the end of the reaction after the data is graphed, the final temperature is determined to be 38.5oC.
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)
a chemist wastes a delicious brownie by burning it in a bomb calorimeter. before burning, the brownie weighed 16.13 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 7.40 degrees celsius. The known heat capacity of the calorimeter that was used was 26.53 kJ/Celsius. What is the energy content, in kJ/g, of this brownie?
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.88 kg sample of C,H0, from 35.8 °C to 51.4 °C. The experiment shows that 2.34 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H00,? Round your answer to 2 significant digits. |J-mol 1 - 1 •K х10
A hot lump of 36.1 g of aluminum at an initial temperature of 51.1 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
A calorimeter contained 81.0 g of water at 16.35°C. A 120.-g sample of iron at 66.60°C was placed in it, giving a final temperature of 19.80°C for the system. Calculate the heat capacity of the calorimeter. Specific heats are 4.184 J/g-°C for H20 and 0.444 Jg-°C for Fe. Heat capacity of the calorimeter = J°C
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?
Part A A silver block, initially at 55.8 °C, is submerged into 100.0 g of water at 24.1°C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.3 °C. The specific heat capacities for water and silver are = 4.18 J/(g ·°C) and 0.235 J/(g·°C). What is the mass of the silver block? Express your answer to two significant figures and include the appropriate units. Cs, water • View Available Hint(s) Cs, silver = HA ? Value Units m =