Activity 3. Calculate the heat evolved when 266 g of white phosphorus (P, ) burns in airaccording to the equation: P+ 50,2 (g)→ P, 010 (s) AH = -3013 kJ/mol4(s) Activity 2. Stoichiometric Calculations involving Enthalpy ChangeThe reaction so,(g) + H,0(1)- H,SO,(aq) is the last step in the commercialproduction of sulfuric acid. The enthalpy change for this reaction is 227 kJCalculate AH for a process in which a 20.0 g so,(g) is allowed to react with excesswater to produce sulfuric acid.

Activity 2 :- it is given that when 1 mole of SO3 react then change in enthalpy of reaction is…

Answered: Activity 3. Calculate the heat evolved…

Activity 3. Calculate the heat evolved when 266 g of white phosphorus (P.) burns in a according to the equation: P + 502 (0) → P, 010 (s) AH = -3013 kJ/mol 4(s)

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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Activity 3. Calculate the heat evolved when 266 g of white phosphorus (P, ) burns in air
according to the equation: P
+ 50,
2 (g)
→ P, 010 (s) AH = -3013 kJ/mol
4(s)

Activity 2. Stoichiometric Calculations involving Enthalpy Change
The reaction so,(g) + H,0(1)
- H,SO,(aq) is the last step in the commercial
production of sulfuric acid. The enthalpy change for this reaction is 227 kJ
Calculate AH for a process in which a 20.0 g so,(g) is allowed to react with excess
water to produce sulfuric acid.

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