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Complete this table relating the values of cell and AG to K cell AG >00 <0
Complete this table relating the values of AGⓇ and K. AG <0 >1 = 1 <1
Complete this table relating the values of E_Cell and DeltaG degree to K.
Complete this table relating the values of E_cell and Delta G to the Q/K ratio.
-6. Calculate the AG for the cell, Ag | Ag+! || Cut? Cu Aggit Cu2+ -> Curst Agron 064.980 Till 77.11-64.98 89.285 AG=128360
Given the electrochemical cell below, answer the following questions. S<H2(g) 00 Ag Agt H+ If the concentration of Agt is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of Hy is 1.00 atm, calculate the cell potential at 25.0°C.
of 25 > Use the data given here to calculate the values of AG at 25 C for the reaction described by the equation Compound A AG (kl/mol) +387.7 - 552.1 +4020 B ABC с AG 537.8 J If AH;, and AS, are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is O entropy driven to the left. Question sur MRG General Chemistry TP SAMSUNG с O O $ %...
( 8 of 12 > - -0-0-0-0-0-0-0-0-0- Table 1. Duration (In minutes) of yeast cell cycle phases in a nutrient-rich environment and a nutrient-poor environment Nutrient-rich environment Nutrient-poor environment Cell Cycle Stages Sand G Mitosis 33 Cytokinesis The cell cycle of yeast cells grown in the nutrientpoor environment is approximately what percent of the cell cycle of yeast cells grown in the nutrienteich environment? A 168 2 160 07:33 9 9
4. What are the mathematical signs/values for E, AG, and K for an electrochemical cell that is spontaneous under standard conditions? 5. Use cell potential data to explain why copper metal does not dissolve in a 1.0 M solution of a typical strong acid, such as HCl, but will dissolve in 1 M nitric acid Cu(s) + 2 H(aq) No Reaction 3 Cu(s) + 2 HNO3(aq) + 6H* 3 Cu?*(aq) + 2NO(g) + 4H2O(1)
QUESTION 25 Match the following Q=K Q<k Q>K A. AG > AG B.DGO C equilibrium D. AGO E. standard state F. AG AG G.K=0 - Q = 1 Q> Q< 1 QUESTION 15 For a reaction at equilibrium, AS univ=0. True False QUESTION 16 As a chemical reaction proceeds toward equilibrium, the free energy of the system decreases. True False QUESTION 17 For a given reaction, a change in the pressure may result in a change in the sign of...
A process at constant T and P can be described as spontaneous if AG <0 and nonspontaneous if AG> 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate AH and AS [assumed independent of temperature and equal to AH° and AS°, respectively] and then use the definition of AG.) 2 MnO2(s) 02(g) 2 MnO(s) AH (kJ mol) -520.0 -385.2 s° (J...