9. Given the following data: 2C1F(g) + O2(g) → Cl2O(g) + F20(g) 2C1F3(g) + 2O2(g) → Cl2O(g) + 3F20 2F2(g) + O2(g)...
At 25°C, the following heats of reaction are known: 2CIF(g) + O2(g) → Cl2O(g) + F2O(g) AHºrn = 167.4 kJ/mol 2C1F3(g) + 202(g) + Cl2O(g) + 3F2O(g) AHºrn = 341.4 kJ/mol 2F2(g) + O2(g) → 2F20(g) AHºrxn=-43.4 kJ/mol At the same temperature, use the above data to calculate the heat released (kJ) when 3.40 moles of CIF(g) reacts with excess F2. CIF(g) + F219) -> CIF3(g) Write answer to three significant figures. NO SIGN in ANSWER. Numeric Response
pter 4-6 0 Saved Help Save At 25°C, the following heats of reaction are known: 2C1F(g) + O2(g) → Cl2O(g) +F20(g) 2C1F3(g) + 2O2(g) + Cl2O(g) + 3F2O(g) 2F2(g) + O2(g) → 2F20(g) AHO/= 167.4 kJ/mol AHºrn = 341.4 kJ/mol AHºrn=-43.4 kJ/mol At the same temperature, use the above data to calculate the heat released (kJ) when 3.40 moles of CIF(g) reacts with excess F2. CIF(g) + F2(9) --> CIF3(9) Write answer to three significant figures. NO SIGN in ANSWER....
AH° = ? 3.(5pts) Consider the thermochemical reaction: CIF(g) + F (g) ----> CIF3(g) Use the following data to determine the value of the missing quantity in the above equation. 2 CIF(g) + O2(g) -----> CI2O(g) + F2O(g) 2 CIF,(g) + 2 O2(g) ----> CI-O(g) + 3 F2O(g) 2 F2(g) + O2(g) -- -> 2 F.0(g) AH AH AH = 167.4 kJ/mol = 341.4 kJ/mol = -43.4 kJ/mol
At 25°C, the following heats of reaction are known: 2CIF(g) + O2(g) → Cl20(g) + F2。dH'm = 167.4 kJ/mol 2ClF3(g) + 202(g) → Cl20(g) + 3F20(g) ΔH'm-34 1.4 kJ/mol 2F2(g) + O2(g) → 2F20(g) ΔHoxn--43.4 kJ/mol At the same temperature, use Hess's law to calculate ΔHorn for the reaction: CIF(g) + F2(g) → ClF3(g) 0 a-21 7.5 kJ/mol O b 465.4 kJ/mol O c. -108.7 kJ/mol d 217.5 kJ/mol O e-130.2 kJ/mol
At 25°C, the following heats of reaction are known: AH (kJ/mol 167.4 2CIF + 02 →Cl20 + F20 2ClF3 + 202 →Cl20+3F20 341.4 2F2 + 02 → 2F20 At the same temperature, calculate ΔH for the reaction: ClF + F2 → CIF3 -43.4 A. -217.5 kJ/mol B.-130.2 kJ/mol C. +217.5 kJ/mol ○ D.-108.7 kJ/mol E. none of these QUESTION 4 Consider the reaction: When a 12.9-g sample of ethyl alcohol(molar mass 46.07 g/mol) is burned, how much energy is released...
3.(5pts)) Consider the thermochemical reaction: 3 CIF(g) + 3F.(g) ---->3 CIF,(g) AHºrn = ? Use the following data to determine the value of the missing quantity in the above equation. 6 CIF(g) + 3 O2(g) ----->3 ClO(g) + 3 F 0(g) 2 CIF3(g) + 2 02(8) -----> CLO(g) + 3 F.0() 2 F2(g) + O2(g) -------> 2 F.O(g) AH AH° AH - 502.2 kJ/mol 341.4 kJ/mol = -43.4 kJ/mol
. Given the following reaction at 25o C. 4NH3(g) + 5 O2(g) 4NO(g) + 6H2O(l) ΔHo = -1168 kJ ΔHo f(NH3) = -46.2 kJ/mol; ΔHo f(H2O) = -285.8 kJ/mol. What is the standard enthalpy of formation of NO gas at 25o C?
Given the following data: 3 s(s) + 2O2(9) S03(9) AH = -395.2 kJ 2802(g) + O2(g) +2503(9) AH = - 198.2 kJ Calculate AH for the reaction: S(s) + O2(g) → SO2(g) +296.1 kJ -197.0 kJ -296.1 kJ -593.4 kJ -494.3 kJ
Use standard enthalpies of formation to determine the ΔHo in kJ for the following reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) ΔHfo (NH3(g)) = -45.90 kJ/mol ΔHfo (NO(g)) = 90.29 kJ/mol ΔHfo (H2O(g)) = -241.83 kJ/mol
(NO(g)) = 20. Determine the enthalpy for the following reaction, given AH (NH3(g)) = -46.1 kJ/mol, AH +90.3 kJ/mol, and AH (H2O(g)) = -241.8 kJ/mol. 4NH3(g) + 502(g) → 4NO(g) + 6H2O(g) AH x = ? kJ a. -1274 kJ/mol d. -905.2 kJ/mol b. -1,996 kJ/mol e. -105.4 kJ/mol c. +1,274 kJ/mol