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- Calculate ΔG0 (in kJ/mol) given ΔG= -423.1 kJ/mol and R= 0.008314 kJ/mol K and T= 611.3 K and Q=0.601ΔG=ΔG0+RTlnQcalculate delta H for the following unbalanced reaction: C6H12O6 + O2 (g) --> CO2 (g) + H2O (g)Calculate ΔG^0 (in kJ/mol) given ΔG= -833.7 kJ/mol and R= 0.008314 kJ/mol K and T= 261.5 K and Q=0.623ΔG=ΔG^0+RTlnQ A) -836 B) -833 C) -834 D) -833 E) -710
- What would be the equilibrium temperature if you drop 5.0 g of brass (Cp= 0.38 J/g-°C, initially at 68°C) and 3.5 g of aluminum (Cp = 0.9 J/g-°Cinitially at 83°C) into 105 g of water (Cp = 4.184 J/g-°C,initially at 23°C)?Plants synthesize carbohydrates from CO2 and H2O by the process of photosynthesis. For example, 6CO2(g)+6H2O(l)C6H12O6(aq)+6O2(g) G=2.87103 kJ at pH 7.0 and 25°C. What is K for the reaction at 25°C?asap plss thsnkassss dsadadawdafa
- What would be the equilibrium temperature (oC) if you drop 5.0 g of brass (Cp = 0.38 J/g-oC, initially at 68oC) and 3.5 g of aluminum (Cp = 0.9 J/g-oC, initially at 83oC) into 20 g of water (Cp = 4.184 J/g-oC, initially at 23oC)?Determine AGrxn for 2 A(g) + B₂(g) → 2 AB(g) A. -400 kJ B. -250 kJ C. -200 kJ D. -100 kJ E. -50 kJ Compound(state) AG (kJ/mol) A(g) B₂(g) AB(g) 0 -100 -150Calculate KK givenEcell= -1.74 voltsE^0cell= -1.16 voltsT= 515 Kelvinn= 1R= 8.314 J/mol KF= 96500 C/mole electronsEcell=E^0cell−RT/nFlnK answer choices: a. 2.04×10^9 b. 2.54×10^3 c. 4.10×10^5 d. 4.75×10^5 e. 4.93×10^0
- What is the equilibrium pressure of O 2(g), in bar, over a sample of NiO(s) at 298 K, given that Δ rG˚ = 218.4 kJ for the reaction: NiO(s) ↔ Ni(s) + ½O 2(g)? Give your answer in scientific notation (e.g. 211 would be 2.11e2)What is ∆G° for the reaction CH₃OH(g) → CO(g) + 2 H₂(g) at 25°C?What would be the equilibrium temperature if you drop 5.0 g of brass (Cp = 0.38 J/g-oC, initially at 68oC) and 3.5 g of aluminum (Cp = 0.9 J/g-oC, initially at 83oC) into 105 g of water (Cp = 4.184 J/g-oC,initially at 23oC)?
