Question: Determine the enthalpy of formation of liquid hydrogen peroxide, H2O2, at 25°C from the following thermochemical equations: Since the equation is not given, you have to write the balanced equation to form I mol H:O: from elements! H2 (g) + ½ O2 (g)→ H20 (g) 2H (g) + ½ O2 (g) → H20 (g) 2H (g) + 2 0 (g) O2 (g) H2O2 (I) H2O2 (g) AH° = -241.82 kJ/mol AH° = -926.92 kJ/mol AH° = -1070.60 kJ/mol AH° = -498.34 kJ/mol - H2O2 (g) 20 (g) → AH° = +52.46 kJ/mol [+60.38 kJ mot')

Question: Determine the enthalpy of formation of liquid hydrogen peroxide, H2O2, at 25°C from the following thermochemical equations: Since the equation is not given, you have to write the balanced equation to form I mol H:O: from elements! H2 (g) + ½ O2 (g)→ H20 (g) 2H (g) + ½ O2 (g) → H20 (g) 2H (g) + 2 0 (g) O2 (g) H2O2 (I) H2O2 (g) AH° = -241.82 kJ/mol AH° = -926.92 kJ/mol AH° = -1070.60 kJ/mol AH° = -498.34 kJ/mol - H2O2 (g) 20 (g) → AH° = +52.46 kJ/mol [+60.38 kJ mot')

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 42QAP: When hydrazine reacts with oxygen, nitrogen gas and steam are formed. (a) Write a thermochemical...

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One step in the manufacturing of sulfuric acid is the conversion of SO2(g) to SO3(g). The thermochemical equation for this process is SO2(g)+12O2(g)SO3(g)H=98.9kJ The second step combines the SO3 with H2O to make H2SO4. (a) Calculate the enthalpy change that accompanies the reaction to make 1.00 kg SO3(g). (b) Is heat absorbed or released in this process?
Give the definition of the standard enthalpy of formation for a substance. Write separate reactions for the formation of NaCl, H2O , C6H12O6, and PbSO4 that have H values equal to Hf for each compound.
Given the following thermochemical equations: 4B(s)+3O2(g)2B2O3(s)H=2543.8kJ H2(g)+12 O2(g)H2O(g)H=241.8kJ B2H6(s)+3O2B2O3(s)+3H2O(g)H=2032.9kJ Calculate H for the decomposition of B2H6 into its elements.
9.73 Without looking up any numerical data or doing calculations, predict whether the enthalpy change for each of the following reactions should he positive, negative, or zero. (a) H2O(l)H2O(s) (b) N2(g)2N(g) (c) CH4(g)+2O2(g)CO2(g)+2H2O(l) (d) CO2(s)CO2(g)
When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2, and liquid water are formed. The reaction absorbs 90.1 kJ of heat. (a) Write a balanced thermochemical equation for the reaction. (b) Using Table 8.3, calculate Hf for calcium cyanamide.
When hydrazine reacts with oxygen, nitrogen gas and steam are formed. (a) Write a thermochemical equation for the reaction. (b) How much heat is evolved or absorbed if 1.683 L of steam at 125C and 772 mm Hg are obtained?
Sodium carbonate, Na2CO3, is used to manufacture glass. It is obtained from sodium hydrogen carbonate, NaHCO3, by heating. 2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) Calculate the standard enthalpy of reaction, using enthalpies of formation (Table 6.2).
You want to determine the value for the enthalpy of formation of CaSO4(s), but the reaction cannot be done directly. Ca(s) + S(s) + 2 O2(g) CaSO4(s) You know, however, that (a) both calcium and sulfur react with oxygen to produce oxides in reactions that can be studied calorimetrically, and (b) the basic oxide CaO reacts with the acidic oxide SO3(g) to produce CaSO4(s) with rH = 402.7 kJ. Outline a method for determining fH for CaSO4(s), and identify the information that must be collected by experiment. Using information in Appendix L, confirm that fH for CaSO4(s) = 1433.5 kJ/mol.
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