CHEMISTRY PLEASE HELP
1)Using the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol
C (s) + 2 F₂ (g) → CF₄ (g) ∆H° = 141.3 kJ/mol 2 C(s) + 2 H₂ (g) →
C₂H₄ (g) ∆H° = -97.6 kJ/mol Determine the enthalpy for the reaction
C₂H₄ (g) + 6 F₂ (g) → 2 CF₄ (g) + 4 HF (g).
2)Using the equations N₂ (g) + O₂ (g) → 2 NO (g) ∆H° = 180.6 kJ/mol N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol 2 H₂ (g) + O₂ (g) → 2 H₂O (g) ∆H° = -483.7 kJ/mol Determine the enthalpy for the reaction 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g).
CHEMISTRY PLEASE HELP 1)Using the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H°...
Question 8 of 20 Using the equations H2(g) + F2 (g) → 2 HF (g) AH° = -79.2 kJ/mol C(s) + 2 F2 (g) → CF. (g) AH° = 141.3 kJ/mol 2 C(s) + 2 H2 (9) C2H4 (9) AH = -97.6 kJ/mol Determine the enthalpy for the reaction C2H4 (g) + 6 F2 (g) → 2 CF4 (9) + 4 HF (g). kJ/mol
Using the equations; N₂ (g) + O₂ (g) → 2 NO (g) ∆H° = 180.6 kJ/mol N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) ∆H° = -91.8 kJ/mol 2 H₂ (g) + O₂ (g) → 2 H₂O (g) ∆H° = -483.7 kJ/mol Determine the enthalpy for the reaction 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g). answer in kJ/mol
Please show all steps and work. ThanksTodd? < Time's Up! View Solution Using the equations H2 (g) + F2 (g) → 2 HF (g) AH° = -79.2 kJ/mol C(s) + 2 F2 (g) → CF4 (g) AH° = 141.3 kJ/mol Determine the enthalpy for the reaction C(s) + 4 HF (g) → CF, (g) + 2 H2 (g). | kJ/mol
Question 36 of 50 Submit Using the equations N2(g) + 3 H2(g) - 2 NH; (g) AH = -91.8 kJ/mol C(s) + 2 H (g) – CH2 (g) AH° = -74.9 kJ/mol H2 (g) + 2c(s) + N2 (g) - 2 HCN (g) AH = 270.3 kJ/mol Determine the enthalpy for the reaction CH, (g) + NH4 () – HCN (g) + 3 H2(g). kJ/mol 1 2 3 C +/- : 0 x 100
5.65 From the enthalpies of reaction H 2 (g)+r 2 (g) longrightarrow2 HF(s) Delta*H = - 537kJ C(s)+2 F 2 (s) longrightarrow CF 4 (g) Delta*H = - 680kJ 2C(s)+2 H 2 (g) C 2 H 4 (g) Delta*H = + 52.3kJ calculate Delta*H for the reaction of ethylene with F 2 : C 2 H 4 (g)+6 F 2 (g) 2 CF 4 (g)+4 HF(g) 5.65 From the enthalpies of reaction H2(8) + (8) 2 HF(8) AH = -537...
Submit Question 33 of 50 For the chemical reaction H2 (g)+ F2 (g) 2 HF (g) AH = -79.2 kJ/mol. What is the enthalpy for the reaction 3 H2 (g)+3 F2 (g) 6 HF (g) kJ/mol 1 2 3 4 5 6 C 8 +- 0 x 100 O 7
Using the equations N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol C(s) + 2 H2 (g) → CH4 (g) AH° = -74.9 kJ/ mol H2 (g) + 2 C(s) + N2 (g) → 2 HCN (g) AH° = 270.3 kJ/mol Determine the enthalpy for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g).
Ammonia will burn in the presence of a platinum catalyst to produce nitric oxide, NO. 4NH_3(g) + 5O_2(g) rightarrow 4NO(g) + 6 H_2 O(g) What is the heat of reaction at constant pressure? Use the following thermochemical equations: N_2(g) + O_2 (g) rightarrow 2NO(g): Delta H = 180.6 kJ N_2(g) + 3H_2 (g) rightarrow 2 NH_3 (g) Delta H = -91.8 kJ 2H_2 (g) + O_2 (g) rightarrow 2H_2O(g): Delta H = -483.7 kJ
Using the standard enthalpy of formation data, show how the standard enthalpy of formation of HF(g) can be used to determine the bond energy. (Enter unrounded values.) (a) bond energy calculated from standard enthalpy of formation kJ/mol (b) average bond enthalpy from the bond enthalpy table k]/mol Average Bond Enthalpies bondAH bond (kJ/mol) bond AHbond (kJ/mol) bond AH bond (kJ/mol) bond AH bond (kJ/mol) O-H 0-0 467 146 495 185 203 156 364 522 335 544 413 347 614 839...
Dok Solutions Chex G tb ofibular syndesmosis articuli X study guide lab practical-Goog x + Question 3 of 20 Using the equations N2(g) + 3 H2(g) - 2 NH3 (9) AH = -91.8 kJ/mol C(s) + 2 H (g) – CHK (g) AH = -74.9 kJ/mol H (g) + 2 C(s) + N (g) + 2 HCN (g) AH = 270.3 kJ/mol Determine the enthalpy for the reaction CH4 (g) + NH3 (g) – HCN (g) + 3 H (g)....