THIS IS Chapter 10 Jeopardy

With Your Host... Ms. Siam

Jeopardy Extras Vocabulary Vocabulary 2 Heat/q=cmt problems ΔH problems Concept Questions 100 100 100 100 100 100 200 200 200 200 200 200 300 300 300 300 300 300 400 400 400 400 400 400 500 500 500 500 500 500

Entropy A 100

A measure of the disorder of a system

Specific heat capacity

Energy needed to raise temperature of 1 g of a substance by 1°C

Calorie A 300

Energy needed to raise the temperature of 1 g of water by 1 °C

Endothermic A 400

Energy as heat flows into system

Exothermic A 500

Energy as heat flows out of system

Surroundings B 100

The remainder of the universe B 100

System B 200

Portion of the universe in which you are interested B 200

Heat B 300

Flow of energy due to temperature differences B 300

Temperature B 400

Measure of the random motions of molecules and atoms of a substance

State function B 500

Property of a system that changes independent of the pathway taken B 500

The amount of energy needed to heat 2. 00 g of carbon from 50 The amount of energy needed to heat 2.00 g of carbon from 50.0°C to 80.0°C is 42.6 J. The specific heat capacity of this sample of carbon is? C 100

0.710 J/g °C C 100

How many joules of energy would be required to heat 24 How many joules of energy would be required to heat 24.2 g of carbon from 23.6°C to 54.2°C? (Specific heat capacity of carbon = 0.71 J/g °C.) C 200

5.3 x 102 J C 200

Assume that 372 J of heat is added to 5.00 g of water originally at 23.0°C. What would be the final temperature of the water? (Specific heat capacity of water = 4.184 J/g °C.) C 300

40.8°C C 300

Calculate how many calories of heat were added to 177 g of copper as it cooled from 155.0°C to 23.0°C. The specific heat capacity of copper is 0.385 J/g °C. C 400

2150 calories C 400

How many calories of heat were added to 5 How many calories of heat were added to 5.0 x 102 g of water to raise its temperature from 25 °C to 55 °C? C 500

1.5 x 104 calories C 500

(pay attention to the wording “is released”) When 1 mole of ethylene (C2H4) is burned at constant pressure, 1410 kJ of energy is released as heat. Calculate ΔH for a process in which 10.0 g of ethylene is burned at constant pressure. (pay attention to the wording “is released”) D 100

-503 kJ D 100

When 1 mole of propane (C3H8) is burned at constant pressure, 2221 kJ of energy is released as heat. Calculate ΔH for a process in which 25.0 g of propane is burned at constant pressure. D 200

-1260 kJ D 200

How much heat is evolved if 25 How much heat is evolved if 25.00 g of methanol (CH3OH) is burned in excess O2? The reaction is 2CH3OH(l) + 3O2(g)  2CO2(g) + 4H2O(g) ΔH = -1453 kJ D 300

566.9 kJ D 300

Given the following data: C(s) + O2(g)  CO2(g) ΔH = -393.5kJ 2CO(g)+O2(g)2CO2(g) ΔH = -566.0 kJ Calculate ΔH for the reaction C(s) + 1/2O2(g)  CO(g) D 400

-110.5 kJ D 400

Given the following data, C(s) + O2(g)  CO2(g) ΔH= -393.5 kJ C2H4(g) + 3O2(g)  2CO2(g) + 2H2O(l) ΔH= -1410.9 kJ H2(g) + 1/2O2(g)  H2O(l) ΔH= -285.8 kJ Calculate ΔH for the reaction 2C(s) + 2H2(g)  C2H4(g) D 500

52.3 kJ D 500

A negative sign for the change in enthalpy for a reaction indicates that the reaction is

Exothermic E 100

One _____ of water requires 4 One _____ of water requires 4.184 J of heat to cause a change in temperature of 1°C E 200

Gram E 200

ΔH for a reaction is the ________ of the enthalpy of the products and the enthalpy of the reactants

Difference E 300

The amount of heat gained or lost by a substance depends on what three things

1.The change in temperature of the substance 2.The mass of the substance 3.The specific heat capacity of the substance E 400

If a reaction is endothermic, do the reactants or the products of the reaction have the higher potential energy content E 500

Products E 500

Define energy F 100

Ability to do work or produce heat F 100

Define potential energy

Stored energy F 200

Define kinetic energy F 300

Energy of motion F 300

Define work F 400

Force acting over a distance

If a piece of aluminum of mass 4. 50 g and temperature 99 If a piece of aluminum of mass 4.50 g and temperature 99.5 °C is dropped into 12.0 g of water at 21.0 °C, what will be the final temperature of the water-aluminum mixture? The specific heat capacity of aluminum is 0.902 J/(g °C) F 500

26.9 °C F 500

Game Designed By C. Harr-MAIT Good luck on the test! Game Designed By C. Harr-MAIT