**Relating Heat, Temperature Change, and Heat Capacity**1. **Scenario:** - Large beds of rocks are used in some solar-heated homes to store heat. Assume that the specific heat of the rocks is 0.82 J/gK. a. **Problem 1:** - Calculate the quantity of heat absorbed by 50.0 kg of rocks if their temperature increases by 12.0 °C. b. **Problem 2:** - What temperature change would these rocks undergo if they emitted 450 kJ of heat?

Given (a) Mass of Rocks ( m ) = 50 kg = 50 × 103 gram…

1. Relating Heat, Temperature Change, and Heat Capacity a. Large beds of rocks are used in some solar-heated homes to store heat. Assume that the specific heat of the rocks is 0.82 J/gK. Calculate the quantity of heat absorbed by 50.0 kg of rocks if their temperature increases by 12.0 °C. b. What temperature change would these rocks undergo if they emitted 450 kJ of heat?

1. Relating Heat, Temperature Change, and Heat Capacity a. Large beds of rocks are used in some solar-heated homes to store heat. Assume that the specific heat of the rocks is 0.82 J/gK. Calculate the quantity of heat absorbed by 50.0 kg of rocks if their temperature increases by 12.0 °C. b. What temperature change would these rocks undergo if they emitted 450 kJ of heat?

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

5. When 1.00g of NaCl (MM 58.44 g/mol) is dissolved in 50.00g of water, the temperature drops by 0.319°C. This temperature change is only detectable by the most sensitive thermometers. If this process takes place in a very well insulated calorimeter, no calorimeter constant is needed. a. Calculate the enthalpy change per gram of NaCl. b. Calculate the enthalpy change per mole of NaCl.
How much heat is needed to raise the temperature of a 2.5 g piece of copper wire from 20. °C to 80. °C? How much heat is needed to increase the temperature of an equivalent mass of aluminum by the same amount? Once heated, which metal will cool faster?
If a 50.0 g piece of brass rod at 98.0°C is placed in 150.0 g of water at 25.0°C, what is the final temperature? Assume that no heat is transferred to the surroundings. The specific heat capacity of water is 4.18 J/g °C. The specific heat capacity of brass is 0.38 J/g °C. 35 79 42 27
5. If you left equal masses of iron and water out in the sun on a hot day, which one would be hotter after 15 minutes? Why?
17. An ice cube is placed in a sealed insulated container of hot water at 80°C. After five minutes, the ice cube disappears. Ice Cube Heat ener Hot Water 5 min. Water Which best describes the change that took place inside the container? The total heat energy in the container was reduced by the ice cube. The hot water lost the same amount of heat energy as the ice cube gained. in the hot water was reduced by kinetic energy in the ice cube. O Heat energy in the ice cube was dissipated into the hot water.
A. How much heat is gained by the water? B. How much heat heat is lost by the zinc metal? C. From the data in this problem, calculate the specific heat of zinc metal.
4 A chemical reaction is run in 450 grams of liquid water, resulting in the water increasing from a temperature of 15 °C to 95 °C. a. Use the equations in your textbook to calculate how much heat is absorbed by the water? b. What is the change in enthalpy for the system? c. What is the change in enthalpy for the surroundings?
Decide whether the statement is True or False
(please type answer no write by hand)
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?
Suppose a boil water notice is sent out advising all residents in the area to boil their water before drinking it or using it for cooking. You need to boil 18.0 L of water using your natural gas (primarily methane) stove. What volume of natural gas is needed to boil the water if only 10.1% of the heat generated goes towards heating the water. Assume the density of methane is 0.668 g/L, the density of water is 1.00 g/mL, and that the water has an initial temperature of 21.4 °C. Enthalpy of formation values can be found in this table. Assume that gaseous water is formed in the combustion of methane.