solid, or to measure the energy of a solution phase reaction. A student heats 65.30 grams of gold to 98.80 °C and then drops it into a cup containing 79.49 grams of water at 21.52 °C. She measures the final temperature to be 23.49 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.67 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of gold. Specific Heat (Au) =| | J/g °C.

solid, or to measure the energy of a solution phase reaction. A student heats 65.30 grams of gold to 98.80 °C and then drops it into a cup containing 79.49 grams of water at 21.52 °C. She measures the final temperature to be 23.49 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.67 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of gold. Specific Heat (Au) =| | J/g °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

The specific heat of a substance is the amount of heat required to raise the temperature of one gram of the substance by one degree Celsius. The relationship between the amount of heat gained or released by a substance and the change in temperature of the substance is given by the equation ?=??Δ?q=m⁢s⁢Δ⁢T where ?q is the heat gained or released, ?m is the mass of the substance, ?s is the specific heat of the substance, and Δ?Δ⁢T is the change in temperature. 1. Rearrange the equation to solve for ?. 2. When a substance with a specific heat of 0.635 J/g⋅∘C0.635 J/g⋅∘C is heated from 25.2 ∘C25.2⁢ ∘C to 71.4 ∘C,71.4⁢ ∘C, it absorbs 422 J422 J of heat. Calculate the mass of the substance.
A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
The temperature of an object increases by 44.1 °C when it absorbs 3761 J of heat. The mass of the object is 355 g. Calculate the heat capacity of the object.
An 84.01 g sample of water at 88.2 °C is mixed in a calorimeter with 43.6 g of water at 23.4 °C. Calculate the final temperature of the water.
A metal X has a a mass of 10.0g and it was heated up to 120.0⁰C, it was then submerged in water that has a mass of 200.0g. The temperature of water increased from 21.0⁰C to 35.0⁰C. Determine the specific heat capacity of metal X. The specific heat capacity of water is 4.18 J/g ⁰C.
A 45.90 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.51°C to 29.10°C. The specific heat capacity of copper metal and water are J and 4.184 J respectively. g• °C 0.387 g• °C Assuming that heat was transferred from the copper to the water and the calorimeter, determine th heat capacity of the calorimeter. Heat capacity of calorimeter =
4. Determine the final temperature of the solution formed when 0.31 g sodium oxide is added to 100 ml water in a calorimeter. Assume that the volume of the resulting solution is 100 ml. The temperature before reaction is 19°C. The heat capacity of the calorimeter is 20J/°C. Suppose that the specific heat and density of the solution are the same as those of water. Write down all the reaction equations needed to solve this exercise.
A 6.61g sample of an unknown salt (MM=116.82g//mol) is dissolved in 150.00g 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 heat for the dissolution reaction of the 6.61 g of salt
150.0 mL of dilute hydrochloric acid is placed in a coffee cup calorimeter. The initial temperature of the solution is recorded to be 14.5°C. A piece of magnesium ribbon of mass 0.575 g is placed in the solution and allowed to react. If the molar enthalpy change for this reaction is -584 kJ/mol, what final temperature would you predict?
2. A sample of nickel is heated to 99.8°C and placed in a coffee cup calorimeter containing 150.0 g water at 23.5°C. After the metal cools, the final temperature of metal and water mixture is 25.0°C. If the specific heat capacity of nickel is 0.444 J/°C a. what mass of nickel was originally heated? Assume no heat loss to the surroundings.
In a simple calorimeter, a piece of metal weighing 48.67 g was heated to 120.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. Is this process endothermic or exothermic? Explain. Show Your Work
A 30.0 g sample of chromium is heated to 100.0 °C in a boiling water bath. The sample is added to a calorimeter charged with 45.0 mL of water at 34.1 °C. The final temperature of the calorimeter contents is 38.5 °C. Calculate the specific heat of chromium.