The table lists the specific heat capacities of select substances. Specific heat capacity (J/g °C) 0.128 0.235 0.385 0.449 0.903 4.184 Substance lead silver copper iron aluminum water An unknown substance has a mass of 18.9 g. The temperature of the substance increases by 16.5 °C when 73.3 J of heat is added to the substance. What is the most likely identity of the substance? water lead O copper O iron O silver aluminum

The table lists the specific heat capacities of select substances. Specific heat capacity (J/g °C) 0.128 0.235 0.385 0.449 0.903 4.184 Substance lead silver copper iron aluminum water An unknown substance has a mass of 18.9 g. The temperature of the substance increases by 16.5 °C when 73.3 J of heat is added to the substance. What is the most likely identity of the substance? water lead O copper O iron O silver aluminum

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 serving of Chocobits cereal is 122 g.A 1.00-g sample of the cereal is burned in a bomb calorimeter that has a heat capacity, C, of 8.50 kJ K-1, causing the temperature to increase from 25.0°C to 25.8°C. Calculate the energy of Chocobits in Calories per serving to three significant figures. 1 Cal = 4.184 kJ
An unknown substance has a mass of 22.5 g. The temperature of the substance increases from 27.9 °C to 45.1 °C when 90.9 J of heat is added to the substance. The table lists the specific heats of select substances. Substance lead silver copper iron aluminum water G B Specific heat [J/(g- °C)] 0.128 0.235 0.385 0.449 0.903 4.184 H MacBook Air N 1 What is the most likely identity of the unknown substance? O aluminum silver D iron water O lead O copper O 2.30 P
Constants | Periodic Table Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: Part B AHm = En,AH: (products)- E n,AH (reactants) For the reaction given in Part A. how much heat is absorbed when 3.50 mol of A reacts? where n represents the stoichiometric coefficients. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) Value Units Submit Previous Answers X Incorrect; Try Again; 29 attempts remaining Provide Feedback Pearson O 1:35 21
The specific heat of lead is 0.128 J/g·°C. How much heat is needed to raise the temperature of 4.90 g of lead by 46.0 °C?
How much heat, in joules and calories, is needed to heat up 253 mL of water from 13.3 °C to 85.2 °C? Assume the density of water to be 1.00 g/mL.
Classify the reaction endothermic or exothermic and give the change in enthalpy of the reaction. CH3OH (1) + 3 O₂ (g) → 2 CO₂ (g) + 4 H₂O (g) Δ Η = -557 kJ The heat energy in the reaction is Select an answer This makes the reaction Select an answer So, the energy would be on the Select an answer side.
A calorimeter is calibrated to have a heat capacity of 441.2 J/°c. 0.143 g of substance X is burned in the calorimeter and raises its temperature from 23.1 °c to 39.5°c. What is the heat of combustion of substance X in J/g?
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
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.45 kg sample of a pure substance from 36.3 °C to 56.3 °C. The experiment shows that 121. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
The specific heat capacity of silver is 0.2386 J/g °C. Assuming no loss of heat to the surroundings or to the calorimeter, determine the final temperature when 100.0 g of silver at 40.0°C is immersed in 60.0 g of water at 10.0°C.
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
When a 6.50 g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature of the water rises from 21.6 to 37.8oC. Was the chemical reaction (dissolving the solid) endothermic or exothermic? How do you know? Write a balanced chemical equation for this process. Determine how many joules of heat (q) were involved in changing the temperature of the water. If the heat that changed the temperature of the water was a result of the chemical reaction, determine the ΔH of the chemical reaction in kJ/mol of sodium hydroxide.