Endothermic Exothermic Answer Bank A chemical change takes place in a container, making it feel cold to the touch. A chemical change takes place in a container, making it feel hot to the touch. Campers burn wood to stay warm at night. Pocket hand warmers, often used by skiers, start out at room temperature. When the air-tight packaging is opened, a substance contained in a cloth pouch reacts with air, and it quickly begins to feel hot. A "cold pack," often used for sports injuries, starts out at room temperature, but squishing the liquid around causes two substances to mix that were originally kept separate. When those substances react, the pack quickly begins to feel cold.

Endothermic Exothermic Answer Bank A chemical change takes place in a container, making it feel cold to the touch. A chemical change takes place in a container, making it feel hot to the touch. Campers burn wood to stay warm at night. Pocket hand warmers, often used by skiers, start out at room temperature. When the air-tight packaging is opened, a substance contained in a cloth pouch reacts with air, and it quickly begins to feel hot. A "cold pack," often used for sports injuries, starts out at room temperature, but squishing the liquid around causes two substances to mix that were originally kept separate. When those substances react, the pack quickly begins to feel cold.

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 is using a calorimeter to determine the specific heat of a metallic sample. She measures out 128.1 grams of her metal and heats it to 79.6 degrees Celsius. Then, she puts the sample into a calorimeter containing 11.47 grams of water at 45.7 degrees Celsius. She measures the temperature of the water in the calorimeter until the number stops changing, then records the final temperature to be 71.4 degrees Celsius. What is the specific heat of the metal? Please answer to three digits after the decimal point.
In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a metal. She heats 18.4 grams of titanium to 98.86°C and then drops it into a cup containing 75.9 grams of water at 23.43°C. She measures the final temperature to be 25.59°C. Assuming that all of the heat is transferred to the water, she calculates the specific heat of titanium to be J/g°C.
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermometer Stirring rod A student heats 66.89 grams of platinum to 99.25 °C and then drops it into a cup containing 83.90 grams of water at 22.41 °C. She measures the final temperature to be 24.37.°C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.72 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of platinum. Metal sample Specific Heat (Pt) =| J/g °C. 02003 Thomeo-BrockaCoe
A piece of metal was placed into a 75.00 grams of water. The temperature of the water increased from 22.02 °C to 25.08 °C. How much heat (in Joules) did the water absorb from the metal? Do not type units into your answer.
The specific heats of two natural substances are shown in the table. Specific Heat Natural Substance Specific Heat Wet Mud 2.5 J/g °C Sandy Clay 1.4 J/g °C A pile of wet mud and a pile of sandy clay are placed next to each other on a sunny day.If the temperature of each pile is equal and allowed to cool in the shade for a few minutes, which substance is likely to show a lower temperature and why? Wet mud, because it released more heat while placed in the sun. Sandy clay, because it absorbed more heat while placed in the sun. Wet mud, because it requires less energy to increase its temperature. Sandy clay, because it needs to release less energy to decrease its temperature.
A cube of aluminum has a mass of 145 grams and its temperature rises from 15.0 oC to 25.5 oC when placed outside in the sun for a period of time. Calculate the amount of heat absorbed. (Specific Heat: CAl = 0.921 J/goC)
A 125.0 g sample of metal at 85.0°C is placed in 165.0 g of water at 18.0 °C. The temperature of the water rose to 23.3°C. What is the specific heat of the metal? This question has a box to place the question-answer, but you will not get any points unless you show your work on your piece of scrap paper. Show the answer with units on the scrap paper. The specific heat of water is 4.184 J/g°C
Carbohydrates serve as a vital source of chemical energy to the human body. Carbohydrates are broken down into smaller units of glucose, among other sugars, providing energy to various muscles and organs, including the brain. On average, for every 9.00 g of carbohydrates consumed, the body will store 153 kJ of energy. Convert this energy value to kilocalories (kcal). 153 kJ = kcal
A 2.50 g sample of zinc is heated, then placed in a calorimeter containing 65.0 g of water. Temperature of water increases from 20.00 °C to 22.50 °C. The specific heat of zinc is 0.390 J/g°C. What was the initial temperature of the zinc metal sample? (final temperatures of zinc and water are the same)
Which of the following is an endothermic process for the system? In each case, the “system” is underlined. Group of answer choices ice cream melting. a hot pack being used to warm a sore muscle. a heat pump being used to warm a house. a candle burning at a dinner table. ice cubes freezing in the refrigerator.
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?