Formula equation: NaOH(ag) + HCl(aq) → Na*(aq) + Cl (aq) + H2O(1) Write the complete ionic equation: Write the net ionic equation: Using the net ionic equation, find the values of heat of formation (AH°;) and plug them into this formula: Theoretical AHrxn = E AH°f products - = E AH°freactants Note: E means "sum"

Formula equation: NaOH(ag) + HCl(aq) → Na*(aq) + Cl (aq) + H2O(1) Write the complete ionic equation: Write the net ionic equation: Using the net ionic equation, find the values of heat of formation (AH°;) and plug them into this formula: Theoretical AHrxn = E AH°f products - = E AH°freactants Note: E means "sum"

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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Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(g)- →C4H₁0(g) ΔΗ° = -125.6 kJ (2) C₂H4(g)- →2C(s) + 2H₂(g) AH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C₂H4(g) + H₂(g) →C4H10(g) kj AH° = ?
26. Calculate the enthalpy change for the reaction below. NO(g) + O(g) →→→ NO₂(g) Given following data: NO(g) + O₂(g) →→ NO₂(g) + O₂(g) 03(g) → 1.50₂(g) 0₂(g) →20(g) AH-198.9 kJ AH = -142.3 kJ ΔΗ = 495.0 kJ
The reaction between HCl and NaOH is represented below. When equal volumes of 1.00 M NaOH and 1.00 M HCl are mixed, 57.1 kJ of heat is released. What would A H be if 2.00 M HCI and 2.00 M NaOH is used instead of 1.00 M? HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) AH = -57.1 kJ/mol... (A) - 28.6 kJ B-85.7 kJ (c) -57.1 kJ D - 114 kJ
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HC1(aq) → 2 MCl,(aq) + 3 H,(g) ΔΗ = -589.0 kJ 2. HCI(g) → HCI(aq) AH2 = -74.8 kJ 3. H,(g) + Cl,(g) –→ 2 HCI(g) AH3 = -1845.0 kJ 4. MCI,(s) → MCl,(aq) AH4 = -262.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl,(g) → 2 MCl,(s) ΔΗ- kJ
Using the provided enthalpy of formation, determine the enthalpy for the reaction: 3A (s)+ 2B (I) ->C (I) + 4D(s) substance AH;° (KJ/mol) A (s) -286
An experiment was conducted to find the heat of neutralisation in an acid - basereaction.A solution was made by dissolving 3.79g of barium hydroxide in 100 mL of water. 30.0 mL of this barium hydroxide solution was reacted with 27.0 mL of a 0.400 mol L-1solution of nitric acid. The heat of neutralisation was calculated to be 51.7 kJ mol-1. Calculate the temperature change and the resultant pH of the solution
5. Reaction Enthalpy. balance and calculate AH for the following chemical equations. AH (kJ/mol): HCN = 130.5, Ca3(PO4)2=-4120.8, H3PO4-1288, SiCl₁=-640.1, SiO₂= -910.9, Mg0=-601.6, HCl=-167.16 d) Mg(s) + H₂0(g) 0 Mg(OH)2(s)
Calculate the change in enthalpy of the following reaction. ΔH (Fe3O4) = -1120.9 kJ ΔH (Al2O3) = -1669.8 kJ 8Al(s) + 3Fe3O4(s) -> 4Al2O3(s) + 9 Fe(s
25.00 mL of 0.4600 M phosphoric acid are reacted with 94.00 mL of 0.7970 M sodium hydroxide. The sodium hydroxide is in excess. Initially, both solutions are at room temperature, 24.692°C. After the reaction is complete, the temperature of the solution has increased to 30.347°C. What is the enthalpy of the reaction in kJ/mol acid? Assume the density of the solution is 1.00g/mL and the specific heat of the solution is the same as water (4.184 J/g-K).
Determine the enthalpy of reaction for HCI(g) + NANO,(s) → HNO,(1) + NaCI(s) 2NACI(s) + H,O(1) → 2HCI(g) + Na O(s) AH° = -507.1 kJ/mol NO(g) + NO,(g) + Na¸O(s) → 2NAÑO,(s) AH° = -427.0 kJ/mol NO(g) + NO,(g) → NO(g) + 0,(g) AH° = -43.01 kJ/mol 2HNO (1) → NO(g) + 0,(g) + H,O(1) AH° = +34.02 kJ/mol