Q.31. To prepare sulfur from hydrogen sulfide extracted from the natural gas, the hydrogen sulfide gas with sulfur dioxide gaseous: we thus obtain liquid sulfur and water steam. 1) Write the equation of this reaction and calculate, using the data, its standard enthalpy at 298K. 2) Explain why the standard enthalpy of formation of liquid sulfur isn't zero? (Explain in one sentence only). Given: Standard molar enthalpies of formation at 298.15K Substance and State AH° (kJ/mol) SO, (g) -298.8 S(1) S(s) +11.8 H,S(g) -20.6 H,O(g) -241.8 H,O(1) -286

Q.31. To prepare sulfur from hydrogen sulfide extracted from the natural gas, the hydrogen sulfide gas with sulfur dioxide gaseous: we thus obtain liquid sulfur and water steam. 1) Write the equation of this reaction and calculate, using the data, its standard enthalpy at 298K. 2) Explain why the standard enthalpy of formation of liquid sulfur isn't zero? (Explain in one sentence only). Given: Standard molar enthalpies of formation at 298.15K Substance and State AH° (kJ/mol) SO, (g) -298.8 S(1) S(s) +11.8 H,S(g) -20.6 H,O(g) -241.8 H,O(1) -286

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

Consider the two reactions. 2 NH, (g) + 3 N,0(g) → 4N,(g) + 3 H,0(1) 4 NH, (g) + 3 0,(g) 2 N,(g) + 6 H,0(1) AH° = -1010 kJ AH° = 1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N, (g) + 0,(g) → N,0(g)
Q.30. Calculate the heat of combustion AH, , 298K of solid oxalic acid (C2H2O4, s) at 25 °C and atmospheric pressure, using the standard molar enthalpies of formation. 1) Write the equation of this reaction and calculate, using the data, its standard enthalpy at 298K. 2) Explain why the standard enthalpy of formation of gaseous oxygen is zero? (Explain in one sentence only) Given: Standard molar enthalpies of formation at 298.15K Substance and State A¢H® (kJ/mol) C2H2O4(s) -829.9 C2H2O4(g) -731.8 CO2(g) -393 CO2(aq) -413.26 H2O(g) -241.8 H2O(1) -285.2 O2(g)
Using Hess’s Law, calculate for the change in enthalpy of the given reactions.
(a) Magnesium reacts with hydrochloric acid to produce hydrogen gas. AH, for HCI(aq) = -167.16 kJ/mol %3D AH", for MgCl(aq) = -801.17 kJ/mol Calculate the standard enthalpy change for this reaction. For this reaction, explain the sign of AT for the surroundings (1) (i) Write the net ionic equation for this reaction What type of reaction is this? In our everyday lives, we observe what happens around us using five biological senses. Give the names of the biological senses. (v) (vi) If you reacted magnesium with hydrochloric acid in the laboratory, specifically what would you observe? Give four observations (b) In the laboratory, what do we wear in different situations to protect ourselves? (c) Give four reasons for working in the fume hood in the laboratory.
Johnson and Steele determined the standard enthalpy of combustion of UO₂(s) in gaseous fluorine. The products of combustion are UF(s) and O2(g). The measured value of the enthalpy of combustion is -1112.6 kJ mol-¹ (per mole of UO₂), and the standard enthalpy of formation of UF(s) is -2197.7 kJ mol-¹. Calculate the standard enthalpy of formation of UO2(s) in kJ mol-¹.
Q.30. To prepare sulfur from hydrogen sulfide extracted from the natural gas, the hydrogen sulfide gas with sulfur dioxide gaseous: we thus obtain liquid sulfur and water steam. 1) Write the equation of this reaction and calculate, using the data, its standard enthalpy at 298K. 2) Explain why the standard enthalpy of formation of liquid sulfur isn't zero? (Explain in one sentence only) Given: Standard molar enthalpies of formation at 298.15K AH (kl/mol) -298.8 Substance and State SO2 (g) S(1) S(s) H-S(g) H2O(g) HO(1) +11.8 -20.6 -241.8 -286
give answer with detail explanation
Background-info: https://drive.google.com/file/d/1G7sPTuESIgWk9wpRdqAnFcsBmOlbBfLv/view?usp=sharing Question: Select each of the following substances for which the standard enthalpy of formation, AH°f, is equal to zero. Assume that all conditions are at standard pressure and temperature. CaO (s) O2 (8) H (aq) Uc(s, graphite) Na e)
Use the standard of enthalpies table to determine the change in enthalpy for: C6H6 (l) + 3/2 O2 (g) --> CO2 (g) + H2O (l) (just balance this equation before you compute for enthalpy change.)
Use the standard of enthalpies table to determine the change in enthalpy for: SO 2(g) + ½ O 2(g) --> SO 3(g)
The standard molar enthalpy of formation for oxygen gas, ?2(?), is zero. The enthalpy of formation for atomic oxygen, ?(?), is +250??/???. Why is there a difference in these values?
Standard Enthalpy of Formations in kJ/mol at 298.15 K ΔHof ΔHof AlCl3(s) -704.2.0 Al2O3(s) -1676 H2O(l) -285.8 H2O(g) -241.8 NH4ClO3(s) -265.2 N2O(g) 81.6 Use data above to calculate the enthalpy change for the reaction: 6Al(s) + 6NH4ClO3(s) => 2Al2O3(s) + 2AlCl3(s) + 3 N2(g) + 12H2O(g) ΔH = ?