3 attempts left Check my work Be sure to answer all parts. From the values of...
From the values of delta H and delta S, predict which of the following reactions would be spontaneous at 26C: Reaction A: delta H = 10.5 kJ/mol, delta S = 30.0 J/K*mol Reaction B: delta H = 1.8 kJ/mol, delta S = -113 J/K*mol If either of the reactions is nonspontaneous, can it (they) become spontaneous? If either of the reactions is nonspontaneous but can become spontaneous, at what temperature might it become spontaneous? Please explain how to do this!
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
html Saved 10 attempts left Check my work Be sure to answer all parts. Determine the amount of heat (in kJ) associated with the production of L46 x 10g of NO, according to- the following equation: 2 NOg)+O2)2NO (g) Enter your answer in scientific notation. AH--114.6 kJ/mol x 10 kJ 2 of 2 <Prev search
2 attempts left Check my work Be sure to answer all parts. For a certain reaction, the frequency factor A is 5.9 x 10° s What is the rate constant for the reaction at 84°C and the activation energy is 16.1 kJ/mol. 3.6 (Enter your answer in scientific notation.)
3 attempts left Check my work Be sure to answer all parts. Isooctane (CgHis; d=0.692 g/mL) is used as the fuel during a test of a new automobile engine. How much energy (in kJ) is released by complete combustion of 29.7 gal of isooctane to gases (AH' = -5.44 x 103 kJ/mol)? Enter your answer in scientific notation. rxn * 10 kJ
3 attempts left Check my work Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as 126) = 2(g) At 1000 K, the equilibrium constant K for the reaction is 3.80 x 10 . Suppose you start with 0.0451 mol of I, in a 2.33-L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of IZ? M What is the equilibrium concentration of I?...
UU Saved Sect 130 10 attempts left Check my work Be sure to answer all parts. Determine the amount of heat (in k.) associated with the production of 2.4410ʻg of NO, according te the following equation: 2 NO() + O2(g) → 2NO2(8) AH =-114.6 kJ/mol Enter your answer in scientific notation. x 10W Typebeto e
3 attempts left Check my work Be sure to answer all parts. Predict whether the entropy change is positive or negative for each of the following reactions. 2 KC104(5) 2 KCIO3(s) + O2(g) positive negative H2O(g) → H20(1) positive negative
2 attempts left Check my work Be sure to answer all parts. A biochemical engineer isolates a bacterial gene fragment and dissolves a 16.0-mg sample in enough water to make 30.0 mL of solution. The osmotic pressure of the solution is 0.340 torr at 25°C. (a) What is the molar mass of the gene fragment? g/mol (b) If the solution density is 0.997 g/mL, how large is the freezing point depression for this solution (K of water = 1.86°C/m)?
8. For the following reaction, CC2(s) + 2H2O(l) + Ca(OH)2(s) + C2H2(g) which is spontaneous at all temperatures, one would predict that a. AG is positive for all temperatures. d. AH is - and AS is for the reaction. b. AH is + and AS is for the reaction. e. AH is + and AS' is- for the reaction. c. AH is - and AS is for the reaction. 9. Calculate the standard absolute entropy, in J/mol K. of Mg:...