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What, specifically?
Heat Stoich!
Hess's Law
Vocabulary
Stuff
100
The specific heat of liquid water?
What is 4.184 J/g deg C? (4.184 J/g K is also OK.)
100
The amount of heat transferred when 2 moles of hydrazine reacts with chlorine according to the following equation: N2H4 + 2 Cl2 --> 4 HCl + N2 delta H = -420 kJ (Specify whether heat is absorbed or released.)
What is 840 kJ released?
100
Change that is applied to the enthalpy change when an equation is reversed.
What is reverse the sign?
100
The capacity for doing work or supplying heat
What is energy?
100
reactants are at higher enthalpy than products. exo or endo?
Exothermic
200
Heat absorbed when 150.0 g of water changes in temperature from 3 deg C to 29 deg C.
What is 16000 J (16 kJ)?
200
The complete, balanced thermochemical equation for the decomposition of two moles of aluminum oxide into aluminum and oxygen gas. In this process 1490 kJ is absorbed. (Be sure to include that energy as either one of the reactants or products.)
What is 2 Al2O3 + 1490 kJ --> 4 Al + 3 O2?
200
Change that happens to enthalpy change if equation is doubled.
What is the delta change is also doubled?
200
The branch of chemistry concerned with the quantities of heat evolved or absorbed during chemical reactions
What is thermochemistry?
200
products at higher enthalpy than reactants. Exo or endo?
Endothermic
300
The final temperature when 372 J of heat is added to 5.00g of water originally at 23.0 degrees C.
What is 40.8 degrees C?
300
What is stoichiometry
Dealing with what amounts of things react with other things.
300
Mathematical operation used to combine both the equations and to determine the overall enthalpy change for the goal reaction.
What is addition?
300
Energy stored in the chemical bonds of a substance
What is potential energy?
300
Energy required to initiate the reaction (get over "the hump" of the enthalpy diagram)
What is the activation energy?
400
The heat transfer, in kJ, when 180 grams of copper cools from 142 deg C to 22 deg C. The specific heat capacity of copper is 0.385 J/g deg C. (Specify whether the energy is being absorbed or released.)
What is 8.3 kJ released?
400
The kilojoules of heat released when 0.75 moles of magnesium burn in an excess of oxygen according to the following equation: 2 Mg + O2 --> 2 MgO + 1204 kJ
What is 450 kJ?
400
The enthalpy change for the reaction IF5(g) → IF3(g) + F2(g) Given the following enthalpies of reaction IF(g) + F2(g)→ IF3(g) ∆H = -390 kJ IF(g) + 2F2(g)→IF5(g) ∆H = -745 kJ
What is 355 kJ?
400
Energy that is transferred from a warm object to a cold object due to a temperature differential
What is heat?
400
Measure of the randomness in the universe
Entropy
500
What is the final temperature of the water and metal (specific heat capacity = 0.52 J/g deg C) of a 12 g metal that is heated to 98 deg C and immersed in 25 g of water in a calorimeter. The initial temperature of the water is 23 degrees C.
What is 27 deg C?
500
The percent yield of an experiment that involves the reaction of 1.48 g of chlorine gas with excess phosphorus that produces 3.00 kJ of heat. 2 P + 5 Cl2 --> 2 PCl5 delta H = -886 kJ
What is 81.1%?
500
The change in enthalpy for the following reaction. 5CO2(g) + Si3N4(s) --> 3 SiO (g) + 2 N2O(g) + 5 CO (g) Given the following two reactions and corresponding enthalpy changes, CO2 (g) + SiO (g) --> SiO2 (s) + CO (g) ΔH = - 520.9 kJ 8 CO2(g) + Si3N4(s)--> 3 SiO2(s) + 2N2O(g) + 8CO(g) ΔH = + 461.05 kJ
What is 2023.75 kJ?
500
The amount of heat needed to increase the temperature of 1g of a substance exactly 1 degree Celsius
What is heat capacity or specific heat.
500
In order to do work, there must be ______ and ______.
force and distance