The value of the equilibrium constant for the following reaction is 4.4. Calculate the concentration of...
Go'=30.5 kJ/mol a) Calculate the equilibrium constant for this reaction at 25C. b) Because deltaGo' assumes standard pH of 7, the equilibrium constant calculated in (a) corresponds to Keq'= [oxaloacetate] [NADH]/ [L-malate] [NAD+] The measured concentration of L-malate in rat liver mitochondria is about 0.20 mM when [NAD+]/[NADH] is 10. Calculate the concentration of oxaloaceteate at pH 7 in mitochondria. c) To appreciate the magnitude of the mitochondrial oxaloacetate concentration, calculate the number of oxaloacetate molecules in a single rat...
Calculate the equilibrium constant K'eq for each of the following reactions at pH 7.0 and 25 °C, using the AG'0 values in the given Table. glucose 6-phosphatase (a) Glucose 6-phosphate + H20 glucose P B-galactosidase (b) Lactose + H20 glucose galactose fumarase fumarateH2O (c) Malate Standard Free-Energy Changes of Some Chemical Reactions AG Reaction type (kI/mol) (kcal/mol) Glycosides MaltoseH,0 Lactose+ H,0 2 glucose glucose +galactose 15.5 15.9 -3.7 -3.8 Rearrangements Glucose 1-phosphate glucose 6-phosphate Fructose 6-phosphate glucose 6-phosphate -7.3 -1.7...
4. Calculate the equilibrium constant in terms of concentration (K) for the following reaction when at equilibrium, there are 0.0406 mol of CH,OH, 0.170 mol of CO, and 0.302 mol of H2 in a 2.00 L container. (Hint: you will have to calculate equilibrium concentrations using moles and volume.) COⓇ) + 2 H20) = CH3OH)
using your average value for the equilibrium constant, calculate the equilibrium NCS- concentration in your solution of "known concentration" Average K = 620.4 Volume of "known concentration" = 0.02L Known Concentration = 10.0mL of 0.05 M Fe(NO3)3 in 1M HNO3, 2.0mL of 0.0005M NaNCS, and 8.0mL of distilled water. (you can assume that all the NCS- is converted to FeNCS2+)
5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the gases at equilibrium for the reaction: CO(g) + H20 (g) = CO2(g) + H2 (g) Given that the initial concentrations of all the gases are 0.05 M and that Kc = 5.1 at 700 K.
30) For the following reaction, the equilibrium concentration of No2 is 0.38 M and equilibrium concentration of N204 is 1.0M, what is the value of the equilibrium constant? 2NO2g) N204() B) 2.6 C) 6.9 D) 0.38 E) 0.14 A) 1.0
For 2.42 For 0.151 Calculate the value of the equilibrium constant for the reaction
Calculate the value of the equilibrium constant Kc for the reaction from the following information: 1st attempt Kc 3.20 C2D Kc = 0.0452
please help answer QUESTION 2 Calculate the value of the equilibrium constant for the following reaction at the indicated conditions: H20H30 (0) OcT(aq) + + HOCI 0.004 M pH 1.044 OCT-0.00455 M (express the answer to 5 decimal places) QUESTION 3 Calculate the equilibrium constant for the following: PbClz (s)PbCl2 (aq) Use the equilibrium constants in appendix 10 and 12. (don't use other sources!!!) NOTE: the Ksp for PbCl2 is incorrect in the textbook tables, but the value for pKso...
A student determines the value of the equilibrium constant to be 1.13x10 for the following reaction. 3Fe2O3(s) + H2(9)—2Fe3O4(s) + H20(9) Based on this value of Keg: AGº for this reaction is expected to be greater, less) than zero. Calculate the free energy change for the reaction of 1.52 moles of Fe,O3(s) at standard conditions at 298K. AGⓇxn = A student determines the value of the equilibrium constant to be 2.34x10-25 for the following reaction. CH (9) + H20(g)—+3H2(g) +...