Reversing the last equation: E + C F The enthalpy is the negative of the enthalpy change of the forward reaction: H = -15 KJ/mol
Now adding the first two reactions and the equation we formed above: 2A + B + D 2F
This means we need to add the individual enthalpies of the three separate equations: -35 + 20 - 15 = -30 KJ/mol
please show neatly with steps thank you. 12) Given the enthalpy changes: 0 Inn A+B →...
Question 12 and 13. Could you please show detailed work. Thank you. 12. Estimate the enthalpy change for the reaction 2CO + O2 → 2CO2 given the following bond energies. BE(C = 0) = 1074 kJ/mol; BEIO = 0) = 499 kJ/mol; BE(C =0) = 802 kJ/mol 13. Using the information given below calculate the H-H bond energy. N2(g) + 3H2(g) + 2NH3(g) AHpX = -105.0 kJ N-N = 160 kJ/mol N=N = 418 kJ/mol NEN = 945 kJ/mol N-H=...
Question 4 of 4 > The enthalpy changes, AH, for three reactions are given. H, ()0,()H,O) Ca(s) +2H (aq) Ca2 (aq) +H,(g) CaO(s) +2H (aq) - AH=-286 kJ/mol AH= -544 kJ/mol Ca2 (aq) +H,O() AH =-193 kJ/mol Using Hess's law, calculate the heat of formation for CaO(s) using the reaction shown. 0,()Ca) Ca(s) + kJ/mol ΔΗ- TOOLS During an experiment, a student adds 1.81 g CaO to 300.0 mL of 1.000 M HCI. The student observès a temperature increase of...
Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D where the heats of formation are given in the following table: Substance ΔH∘f (kJ/mol) A -275 B -413 C 223 D -521 Express your answer in kilojoules. - Part A Calculate the standard enthalpy change for the reaction 2A+B=2C+2D where the heats of formation are given in the following table: Substance A AH (kJ/mol) -275 -413 223 -521 B D Express your answer in kilojoules. View Available Hint(s) O AED *...
I keep getting the answer wrong please show steps! Part A The change in enthalpy (AH) for a reaction is -23.5 kJ/mol. The equilibrium constant for the reaction is 2.1x103 at 298 K What is the equilibrium constant for the reaction at 605 K? Express your answer using two significant figures. Submit Request Answer
Given the thermochemical equations A(g) — Bg AH = 70 kJ B(g) — C(g) AH = -140 kJ find the enthalpy changes for each reaction 3 A(g) — 3Bg AH = B(g) Ag) AH = A(g) -C(O) AH =
Please SHOW ALL WORK AND STEPS do not skip anything. Thank you(: And write NEATLY thank you Fall 2015 4 13 CHI C. aim
Please show steps on how to solve this problem. Thank you for your time The enthalpy of vaporization of potassium is 89.6 k]/mol and the entropy of vaporization of potassium is 77.5 J/K mol. What is the boiling point of potassium?
5-7 help please !! due soon S When 7.0 g of sodium hydroxide (NaOH) is dissolved in 238.5 g of water in an insulated container, the temperature rises from 20.00 oC to 27.66 oC. Calculate the molar enthalpy change (AH) for the dissolution process in kJ/mol NaOH A) -43.7 kJ/mol B) +45.0 kJ/ml C)-32.7 kJ/mol D) +32.7 kJ/mol E) -45.0 kJ/mol 6) Given the data in the table below, AH rxn for the reaction 4NH3 (g)+502 (8) -- 4NO (g)...
A set of chemical equations and their associated enthalpy values are given. | Reaction A+B → C D +C AH (kJ/mol) 67.5 53.3 | Using this information, write a reaction with an enthalpy of 14.2 kJ/mol. reaction:
CHANGES IN ENTROPY OF UNIVERSE VS SYSTEM. Evaluating Spontaneity Considering both Entropy and Enthalpy 7. In a spontaneous process, which of the following always increases? a. the entropy of the system b. the entropy of the surroundings c. the entropy of the universe d. the entropy of the system and the universe c. the entropy of the system, surroundings and the universe (Hand S refer to the system), a. AH>0 8. Processes are always spontaneous, regardless of temperature, when and...