The change in enthalpywhen one mole of acompound forms from itsconstituent elements intheir standard states.The difference in enthalpybetween two states of asystem.A function whose valuedepends only on the stateof the system. not on howthe system got to thatstate.1Endothermic reactionA chemical reaction thatreleases heat to itssurroundings.2. EnthalpyA chemical reaction that3. Enthalpy changeabsorbs heat from itsSurToundings.4. Exothermic reactionThe enthalpy change for achemical reaction5. Hcat of reactionThe sum of the internal6. Hcss s Lawenergy of a system and theproduct of its pressure andvolume.7 Standard enthalpy of formation8. Standard stateThe law stating that if achemical equation can be9 State functionexpressed as the sum of aserics of steps, then AHfor the overall equation isthe surn of the heats ofreactions for cach step.For a pure gas at a pressLreof cxactly 1 atm: for a pureliquid or solid. its moststable form at 1 atm andthc temperturc ofinterest fora solution VIH000000 constituent elements intheir standard states.The difference in enthalpybetween two states of asystem.A function whose valuedepends only on the stateof the system, not on howthe system got to thatstate.1. Endothermic reactionA chemical reaction thatreleases heat to its2. Enthalpysurroundings.A chemical reaction that3. Enthalpy changeabsorbs heat from itssurroundings.4. Exothermic reactionThe enthalpy change for a5. Heat of reactionchemical reactionThe sum of the internal6. Hess's Lawenergy of a system and theproduct of its pressure and7. Standard enthalpy of formationvolume.8. Standard stateThe law stating that if achemical equation can be9. State functionexpressed as the sum of aseries of steps, then AH,for the overall equation isthe sum of the heats ofreactions for cach step.For a pure gas at a pressureof exactly 1 atm: for a pureliquid or solid, its moststable form at 1 atm andthe temperatiureinterest: for a solution witha concentration of exactly1 M.00000

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The change in enthalpy when one mole of a compound forms from its constituent elements in their standard states. The difference in enthalpy between two states of a system. A function whose value depends only on the state of the system. not on how the system got to that state. 1 Endothermic reaction A chemical reaction that releases heat to its 2. Enthalpy surroundings. A chemical reaction that 3. Enthalpy change absorbs heat from its SUrToundings. 4. Exothermic reaction The enthalpy change for a chemical reaction 5. Hcat of reaction The sum of the internal 6. Hcss s Law energy of a system and the product of its pressure and volume. 7 Standard enthalpy of formation 8. Standard state The law stating that if a chemical equation can be 9 State function expressed as the sum of a serics of steps, then AH for the overall equation is the surn of the heats of reactions for cach step. For a pure gas ac a pressure of cxactly 1 atm: for a pure liauid or solid. is most stable form at 1 stm and Lhe temperature of interest fora solution WVITH 0000

The change in enthalpy when one mole of a compound forms from its constituent elements in their standard states. The difference in enthalpy between two states of a system. A function whose value depends only on the state of the system. not on how the system got to that state. 1 Endothermic reaction A chemical reaction that releases heat to its 2. Enthalpy surroundings. A chemical reaction that 3. Enthalpy change absorbs heat from its SUrToundings. 4. Exothermic reaction The enthalpy change for a chemical reaction 5. Hcat of reaction The sum of the internal 6. Hcss s Law energy of a system and the product of its pressure and volume. 7 Standard enthalpy of formation 8. Standard state The law stating that if a chemical equation can be 9 State function expressed as the sum of a serics of steps, then AH for the overall equation is the surn of the heats of reactions for cach step. For a pure gas ac a pressure of cxactly 1 atm: for a pure liauid or solid. is most stable form at 1 stm and Lhe temperature of interest fora solution WVITH 0000

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...

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A 30.0 g sample of chromium is heated to 100.0 °C in a boiling water bath. The sample is added to a calorimeter charged with 45.0 mL of water at 34.1 °C. The final temperature of the calorimeter contents is 38.5 °C. Calculate the specific heat of chromium.
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3. Suppose the 25.0 g of the following substances all initially at 27.0 °C absorb 2.35 kJ of energy. What is the final temperature of each? D) Water. You will need to look up specific heat values.
1. Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, the methane was extinguished and final measurements were made. = 7.52 g = 7.20 g Mass of methane before burning Mass of methane after burning Mass of water in container Initial temperature of water Final temperature of water = 140.0 g = 10.0°C = 32.0°C a) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from the methane was absorbed by the water b) Write the thermochemical equation for the complete combustion of methane.
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.A student heats 62.45 grams of platinum to 99.18 °C and then drops it into a cup containing 84.71 grams of water at 23.23 °C. She measures the final temperature to be 25.02 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.66 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of platinum.
Define standard enthalpy of combustion. * A. The enthalpy changes of a reaction carried out at standard conditions. B. The enthalpy changes when pure substance is completely burned in excess oxygen at standard condition C. The enthalpy changes when 1 mole of pure substance is completely burned in excess oxygen at standard condition. D. The enthalpy change (heat liberated or absorbed) when one mole of a pure compound is formed from its elements at a standard condition.