The value of AH° for the reaction below is -186 kJ mol-1. H₂ (g) + Cl2 (g) → 2HCl (g) Calculate AH°f for HCl (g). O a. -1.27 × 102 kJ mol-1 O b. -93.0 kJ mol-1 ○ c. +186 kJ mol-1 O d. -3.72 x 10² kJ mol-1 e. -186 kJ mol-1

Given AH = +90.7 kJ/mol and AS = +221.0 J/mol K, determine AG for the reaction CH3OH(g) → CO(g) + 2 H₂(g) at 25.0°C? O a. 12.4 kJ/mol O b. 78 kJ/mol O c. 50 kJ/mol O d. 24.8 kJ/mol O e. 100 kJ/mol revious page

The Δ?vapΔHvap of a certain compound is 42.97 kJ·mol−142.97 kJ·mol−1 and its Δ?vapΔSvap is 76.35 J·mol−1·K−1.76.35 J·mol−1·K−1. What is the boiling point of this compound?

Chemistry

I am confused by only K value. I think it is  Substituting the values: ln(K) = -(-3.9 × 105 J/mol) / (8.314 J/K.mol × 298 K)  = 157.41 Taking the exponential of both sides gives: K = e^157.41  K =  2.3 X 10^68

Without doing any calculations, match the following thermodynamic properties with their appropriate numerical sign for the following exothermic reaction. C,H4(g) + H20(g) →CH3CH,OH(g) Clear All > 0 AHrxn 0 low T, 0 high T Previous Next

For a particular reaction at 150.5 °C, AG = –392.62 kJ/mol, and AS = 692.39 J/(mol · K). Calculate AG for this reaction at -0.4 °C. - AG = kJ/mol 80 DII DD F3 F4 F7 FB F9 F10 F12 %24 & 4. 5 6 7 8 Y U H K F.

Calculate the value of K for the formation of NO2 from NO and O2 at 298 K if ∆?° = -35.3 kJ/ mol for the following reaction. (R = 8.314 J/mol. K) NO(g) + 12 O2 (g) ⇌ NO2 (g)

9. Use the AH°f and AH°rxn information provided to calculate AH°f for IF. Provide the formation reactions that gave rise to the AHºf values. Why is the AHºf value for 12(g) zero? IF7(g) + 12(s)→ IFs(g) + 2 IF(g) AH°rxn = -89 kJ AH (kJ/mol) IF7(g) -941 IFs(g) -840

The value of AH° for the reaction below is -336 kJ. Calculate the heat (kJ) released to the surroundings when 23.0 g of HCl is formed. 26. CH4 (g) + 3Cl, (g) → CHC1; (1) + 3HC1 (g) A) B) C) 211 177 70.7 D) -336