An unknown metal has a mass of 88.0 g. When 2440 J of Metal Specific heat (J/g • C) heat are added to the sample, the sample temperature aluminum 0.897 changes by 30.9 °C. Calculate the specific heat of the tin 0.210 unknown metal. strontium 0.301 barium 0.204 calcium 0.650 specific heat: J/(g · °C) calcium 0.650 What is the possible identity of the metal based on the calculated specific heat? aluminum strontium calcium O tin

An unknown metal has a mass of 88.0 g. When 2440 J of Metal Specific heat (J/g • C) heat are added to the sample, the sample temperature aluminum 0.897 changes by 30.9 °C. Calculate the specific heat of the tin 0.210 unknown metal. strontium 0.301 barium 0.204 calcium 0.650 specific heat: J/(g · °C) calcium 0.650 What is the possible identity of the metal based on the calculated specific heat? aluminum strontium calcium O tin

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 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 is the total mass inside the calorimeter in grams?
105 mL of H2 O is initially at room temperature (22.0° C). A chilled steel rod at 2.0° C is placed in the water. If the final temperature of the system is 21.3 °C, what is the mass of the steel bar? Specific heat of water = 4.18 J/g.°C Specific heat of steel = 0.452 J/g.°C
You take 126 g of a solid (melting point = 48.5 °C, heat of fusion = 514 J/g) and let it melt in 555 g of water. The water temperature decreases from its initial temperature to 52.3 °C. Ignoring the specific heat of the solid, calculate the initial temperature of the water.
q represents the change in heat of a reaction or substance. The units of q are Joules (J) or kilojoules (kJ). For a well understood substance, we can calculate the specific heat which relates the mass of the substance in grams to the amount of heat in J required to raise that amount a certain temperature. We call that specific heat. The specific heat (Cs) of water is stated in the following way: C s ( H 2 O ) = 4.186 J g ∘ C This means that it takes 4.186 J of energy to raise the temperature of 1g of water by 1ºC. The relationship between q and Cs for a given substance is where m is mass (g) and ∆T is the change in temperature in ºC (final temp - initial temp). Calculate the heat change (q) in J when 4.297 grams of water is cooled from 3.967 ºC to -2.902 ºC. Enter your answer with one decimal place (tenths). Pay careful attention to the sign of your answer. The sign of ∆T is always the same as the sign for q.
In a popular television series, the two characters use thermite to assist with breaking into a chemical storage facility because the reaction between aluminum and iron(III) oxide produces a tremendous amount of heat. If they began with 10.0 g of Al, how many kJ of heat would be released? 29. 2 Al(s) + Fe,O3(s) → Al,O;(s) + 2 Fe(s) AH = -852 kJ 158 kJ A) B) 236 kJ 472 kJ D) None of the above
In a coffee-cup calorimeter, 59.0 mL of 0.100 M AgNO3 and 59.0 mL of 0.100 M HCI are mixed to yield the following reaction. Ag (aq) + Cl(aq) → AgCl(s) The two solutions were initially at 19.10°C, and the final temperature is 19.90°C. Calculate the heat that accompanies this reaction in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 118.0 g and has a specific heat capacity of 4.18 1/°C 9- 407 kJ/mol
A piece of metal weighing 146.7 g was heated from 32.0 °C to 56.2 °C. If the amount of heat needed was 1363.3 J, calculate the specific heat of the metal. What is the identity of the metal? 20 Specific Heats of Selected Metals Smetal, J/g-°C Metal 0.901 Smetal, J/g-°C 0.449 Metal Al Fe Cu 0.384 Ni 0.444 Si 0.711 Sn 0.226 Zn 0.389 Mn 1.02
A glass contains 250.0 g of warm water at 78.0°C. A 50.0 g piece of gold at 2.30°C is placed in the water. What is the final temperature reached by this system? The specific heat of water is 4.184) g1 °C1, and that of gold is 0.129J g1 °C1. A 78.45°C B 76.36°C c) 79.63°C D 77.54°C
The density of aluminum is 2.7 g/cm3 and its specific heat is 0.9 J/g.0. A piece of 9.7 cm3 aluminum with an initial temperature of 125 0C is put in 120 g of water in an insulating container with a temperature of 18 0C. What will be the final temperature of the aluminum-water mixture? (Specific Heat of Water: 4.186 J/g.0C)
When a sample of titanium was supplied 1.00 kJ of energy, the temperature rose 103.5 °C. If the specific heat of titanium is 0.523 J/g · °C, what is the mass of the titanium sample?
The specific heat of substance C is 0.93 J/(g K) and that of substance D is 1.8 J/(g K). You are given an unknown that could be pure substance C, pure substance D, or a homogeneous mixture of C and D. In the lab you determine that it requires 23.3 J of heat energy to raise the temperature of a 25.0 g sample of the unknown by 1.0 K. What conclusions can you make about the identity of your unknown, from this data?
What is the heat of a reaction, in joules, with a total reaction mixture volume of 67.3 mL if the reaction causes a temperature change of 5.9 °C in a calorimeter? Assume that the reaction mixture has a density of 1.00 g/mL and a specific heat of 4.184 J/g-°C. The calorimeter has a heat capacity of 10.0 J/°C.