Consider the following equations.
3 A + 6 B → 3 D, ΔH = -440. kJ/mol
E + 2 F → A, ΔH = -102.5 kJ/mol
C → E + 3 D, ΔH = +64.5 kJ/mol
Suppose the first equation is reversed and multiplied by 1/6, the second and third equations are divided by 2, and the three adjusted equations are added. What is the net reaction?
Consider the following equations. 3 A + 6 B → 3 D, ΔH = -440. kJ/mol...
Consider the following equations: 3A + 6B --> 3D ΔH = -403 kJ/mol E + 2F --> A ΔH = -105.2 kJ/mol C --> E + 3D ΔH = +64.8 kJ/mol Suppose the first equation is reversed and multiplied by 1/6, the second and third equations are divided by 2, and the three adjusted equations are added. What is the net reaction and what is the overall heat of this reaction
1) State what is the net reaction. 2) What is the value for ΔH° for the net reaction? (kJ) Consider the following thermochemical equations: (1) CH2OH() + O2(g) HCHO2(/) + H2O(1) AH°= -411 kJ (2) CO(g) + 2H2(g) –CH2OH() AH°=-128 kJ (3) HCHO2(1) CO(g) + H2O(1) AH°= -33 kJ Suppose Equation (1) is reversed and divided by 2; Equations (2) and (3) are multiplied by V2, and then the three adjusted equations are added.
Consider the following two reactions: A → 2B ΔH°rxn = 456.7 kJ/mol A → C ΔH°rxn = -22.1 kJ/mol Determine the enthalpy change for the process: 2B → C Question 40 options: A) 434.6 kJ/mol B) -434.6 kJ/mol C) -478.8 kJ/mol D) 478.8 kJ/mol E) More information is needed to solve the problem.
Using the equations 2Sr(s)+O2(g) → 2 SrO (s) ΔH° = -1184 kJ/mol SrO (s) +CO2 (g) → SrCO3 (s) ΔH° = -234 kJ/mol CO2 (g) → C(s) +O2 (g) ΔH°= 394 kJ/mol Determine the enthalpy for the reaction 2 SrCO3 (s) → 2 Sr (s)+2 C(s)+ 3O2 (g). kJ/mol
Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g) What are the equilibrium constants Kp and Kc for the reaction at 350 K ? You may assume that ΔH∘ and ΔS∘ are independent of temperature.
Consider the following reactions: B(g ) → A(g) ΔH = 27.9 kJ and C(g) → 2B (g) ΔH = -18.0 kJ A. Calculate ΔH for the reaction 4A(g) →4 B(g) B. Using the two equations given Show how you would arrange the reactions so they add up to the equation 2A (g) → C (g), and then calculate ΔH for 2A (g) → C (g)
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? ΔH°f (kJ/mol): -75 -134 -92 A. +662 kJ B. +117 kJ C. -151 kJ D. -335 kJ The equation that corresponds to the enthalpy of formation for NH3(g) is A. N(g) + 3H(g) → NH3(g) B. N(g) + 3/2 H2(g) → NH3(g) C. 1/2 N2(g) + 3H(g) → NH3(g) D. 1/2 N2(g) + 3/2 H2(g) →...
a. b. Consider the follow equations: A+B →D AH° = -70.0 kJ E +2 F → A AH° = -20.0 kJ C + E +2D AH° = -300.0 kJ Calculate the AHⓇ for the reaction: C+2 F → 3 A +2 B Calculate the enthalpy of reaction for the process: D+FG+M A + B + C +G AH° = 100.0 kJ AC+F AH° = -300.0 kJ D+M+B AH° = -150.0 kJ
ΔH f f ° = -36.40 kJ/mol and S° = 245.91 J/mol K for CH 3 3 Br, determine the Gibbs free energy in kJ from the ΔH f f ° and S° values for the reaction CH 4 4 + Br 2 2 → CH 3 3 Br + HBr at 298 K. Give only the numerical part of your answer; i.e., don’t include units in your response.
The standard enthalpy of formation of CO(g) is −111 kJ/mol [refer to this equation C(s) + 1/2O2(g) ⟶ CO(g)] What is the ΔHorxn of this reaction? (What is the standard enthalpy change of this reaction?) 2C(s) + O2(g) ⟶ 2CO(g) -253 kJ/mol - 222 kJ/mol -97.1 kJ/mol 534 kJ/mol 124.9 kJ/mol -50.5 kJ/mol 5 points QUESTION 2 (assume A, B, C, and D and E are chemicals) Look at these equations A + B à C ΔH° = -9 kJ/mol rxn...