In an experiment, 30.0 g of metal is heated to 98.0°C and then quickly transferred to 50.0 g of water in a calorimeter at 27.0°C. The heat capacity of the calorimeter with the water is 211 J/°C. The final temperature comes to 32.5°C. What is the approximate specific heat capacity of the metal? [C>(water) = 4.18 J/(g · °C)] 0.591 J/(g · °C) b. 29.5 J/(g · °C) 0.540 J/(g · °C) d. 0.140 J/(g · °C) e. 83.0 J/(g · °C) a. c.

In an experiment, 30.0 g of metal is heated to 98.0°C and then quickly transferred to 50.0 g of water in a calorimeter at 27.0°C. The heat capacity of the calorimeter with the water is 211 J/°C. The final temperature comes to 32.5°C. What is the approximate specific heat capacity of the metal? [C>(water) = 4.18 J/(g · °C)] 0.591 J/(g · °C) b. 29.5 J/(g · °C) 0.540 J/(g · °C) d. 0.140 J/(g · °C) e. 83.0 J/(g · °C) a. c.

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 student transferred 50.0 ml 1.00 M HCl into a coffee-cup calorimeter, which had a temperature of 25.5 °C. He then added this to 50.0 ml 1.00 M NaOH which also had a temperature of 25.5 °C and stirred the mixture quickly. The resulting solution was found to have a temperature of 32.5 °C. The calorimeter constant for the coffee-cup calorimeter used was 15.0 J/°C. Calculate the heat of reaction. Please include the full solution.
When 15.8 g KBr(s) dissolves in 119.7 g of water at 24.2°C, the final temperature of the solution comes to 21.1°C. Assume the heat capacity of the solution is roughly 4.18 J/(g·°C). What is the molar enthalpy of a solution of potassium bromide (119.00 g/mol)?
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?
The reaction of zinc with hydrochloric acid is represented by the reactionZn(s) + 2 HCl(aq) ↔ ZnCl 2(aq) + H 2(g) -- ΔH = -152.5 kJ How many grams of zinc reacted with an excess of HCl (100.0 mL) if the temperature of the calorimeter increased from 25.0Â°C to 35.85 Â°C? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*Â°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
A 5.1-gram piece of gold jewelry isremoved from water at 100.0°C and placed in a coffee-cup calorimeter containing 16.9 gof water at 22.5°C (specific heat of water is 4.184 J/g · °C). The equilibrium (final)temperature of the water and jewelry is 23.2°C. The calorimeter constant is known fromcalibration experiments to be 1.54 J/°C. What is the specific heat (in J/g · °C) of this pieceof jewelry? If the tabulated value of the specific heat of gold is 0.129oC, is the jewelrypure gold?
A 32.1 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 25.8°C. Calculate the mass of water in the calorimeter.
A piece of chromium metal with a mass of 24.50 g is heated in boiling water to 98.3 °C and then dropped into a coffee-cup calorimeter containing 82.3 g of water at 23.4 °C. When thermal equilibrium is reached, the final temperature is 25.7 °C. Calculate the specific heat capacity of chromium. (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.)
Solid calcium chloride dissolves in water according to the equation below.CaCl2 (s) ➝ Ca+2 (aq) + 2 Cl – (aq) ΔHº = –81.3 kJ/mol8.00 grams of solid CaCl2 dissolves in 45.0 grams of water initially at a temperature of 20.00 ºC in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g·ºC)]Tfinal = Answer ºC
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol
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 =