Your instructor tells you that you only have 0.01 mole of CH3OH which is the limiting reactant and ask you to calculate the equilibrium constant using the free energy to 2 decimal places. Hint: remember there are 2 moles of CH3OH so the free energy calculate is for 2 moles of CH3OH and not per mole CH3OH 2CH3OH(L) + 302(8) 2CO2(g) + 4H20(3)

Your instructor tells you that you only have 0.01 mole of CH3OH which is the limiting reactant and ask you to calculate the equilibrium constant using the free energy to 2 decimal places. Hint: remember there are 2 moles of CH3OH so the free energy calculate is for 2 moles of CH3OH and not per mole CH3OH 2CH3OH(L) + 302(8) 2CO2(g) + 4H20(3)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The standard reaction free energy AG =-64. kJ for this reaction: C(s) + 2Cl₂(g) →CCl4(9) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction C(s) + = C₁₂(g) → 4 CC₁₂ (8) 2CC1 (g) 2C(s) + 4Cl₂ (g) CC1₂(g) → C(s) + 2Cl₂(g) AG KJ KJ KJ x10 Ś
Your instructor tells you that you only have 0.01 mole of CH3OH which is the limiting reactant and ask you to calculate the equilibrium constants using the free energy to 2 decimal places.
I need help with calculating You wish to determine if a certain biochemical reaction will be spontaneous. You have determined the following for this reaction: G(products) = 48 kCal/mole G(reactants) = 12 kCal/mole You have also determined that there are 4 molecules of ATP that can be used in this reaction (ΔG for one ATP = -7.3 kCal). What the ΔG for this biochemical reaction using this level of ATP hydrolysis? .... kCal/mol Will this reaction proceed spontaneously with this level of ATP hydrolysis? ....
What statement is true? During an endothermic reaction the entropy of the surroundings increase. Reactions with a negative ΔGo value are always exothermic. The value of ΔG does not depend on temperature. The symbol that represents the free energy change for a reaction at standard state conditions is ΔGo
Use standard enthalpy and entropy data value from the Table: to calculate the standard free energy change for the reaction shown here (298 K). What does the computed value for ΔG° say about the spontaneity of this process? C2H6(g) ⟶ H2(g) + C2H4(g)
The reaction A + B <> C has a molar DSrxn of -19 J/K and a molar DHrxn of 15 kJ. C has a free energy of formation of 10,000 kJ/mole, and B's free energy of formation is -3500 kJ/mole. What is the free energy of formation of A? Assume standard conditions, choose the closest. -7200 kJ/mole -5700 kJ/mole 7200 kJ/mole 5700 kJ/mole -34100 kJ/mole
A student determines the value of the equilibrium constant to be 7.49×10-37 for the following reaction. H,S(g) + 2H2O(1)3H2(g) + SO2(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.03 moles of H,S(g) at standard conditions at 298K. AG. rxn kJ
From the following data, calculate ΔH° for the reaction O3(g)+NO(g)-->O2(g)+NO2(g) O3 = 142.7 kj/mol NO = 90.3kj/mol O2=0kj/mol NO2= 33.2kj/mol
5. What can be interpreted if only given the following? C6H12O6(s) ----> C6H12O6(aq) The enthalpy of the reaction is negative. The enthalpy of the reaction is positive. The entropy of the reaction is negative. The entropy of the reaction is positive. Not enough information is provided to make any predictions.
The difference in standard free energy between reactant R and product P is + 7.5 kJ/mol. What’s the ratio of P to R at equilibrium? P to R ratio =
A student determines the value of the equilibrium constant to be 6.04x10-37 for the following reaction. 2N2(g) + O2(g) 2N20(g) ht Based on this value of Keg: than zero. AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 2.09 moles of N2(g) at standard conditions at 298K. AG°rxn kJ
For a particular chemical reaction, the standard enthalpy change is -396.5 kJ/mol and the standard entropy change is -333.8 J/K•mol. Calculate the standard free energy change in kJ/mol for this reaction at 25°C. Enter your answer with one decimal place and no units. Example: -23.4