Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Select one: O a. None of the above pairs will react O b. Li*(aq) + Al(s) С. Fe3+(aq) + Ni(s) O d. Pb2+(aq) + Cu(s) O e. Ag*(aq) + Br (aq)

Question 6 Calculate the AG for the following process at 100 K and 300 K. Use the thermodynamic data from Appendix G in OpenStax Chemistry, 2e. If one exists, calculate the temperature (in K) at which the process switches between spontaneous and non-spontaneous. ZaCl() Zn (aq) + 2 Cl (ag) Report G to the tenths place. AG T= " K ப P

Using the appendix informa=on in your textbook calculate E° from ΔG° for the following reaction:CH3OH(l) + 3/2O2(g) ➝ CO2(g) + 2H2O(l)As the temperature increases would you expect E to increase or decrease. Justify your response.

3. If 20 g of KNO3 is dissolved in 50 mL of water at 4 °C, is the system in equilibrium? If not, what spontaneous process will occur? What is the value of AG (NOT AG) for the system, as prepared, before any reaction occurs? KNO3, K², NO₂ (44) NO3(aq) AH R

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.     Zn(s) + Na+(aq)     Sn4+(aq) + Zn(s)     Ni(s) + Ba2+(aq)     Cr3+(aq) + Sn(s)     None of the above pairs will react.

True or false? Why?

What is the equilibrium constant at 25.00°C for the reaction below?  Pb(s) + 2 NiO(s) → PbO2(s) + 2 Ni(s)   ΔG° = 206.1 kJ/mol

A Moving to another question will save this response. Question 13 Under standard conditions, a positive value of AG° for a reaction indicates that: O the reaction is at equilibrium O the reaction is non-spontaneous in the forward direction O the reaction favors formation of products O the reaction is spontaneous in the forward direction O the reaction cannot reach equilibrium A Moving to another question will save this response. MacBook Air esc F2 F3 F4 F5 F1 @ #3 %$4 7 3 4. 6 W R. Breathe easy.

Describe each  reaction  as spontaneous or non-spontaneous. Au^3+  +  Fe^3+ -----> Fe^2+  +  Au

true or false