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If Al3+(aq) = 0.36 M, Sn4+ (aq) = 0.086 M and Sn2+(aq) = 0.54 M, calculate the Ecell of this non standard cell Use: Al3+(aq)  +  3e-  ↔  Al(s)            Ecell = -1.676 V Sn4+(aq)  +  2e-  ↔  Sn2+(aq)  Ecell = 0.154 v

Based on the Gibbs free energy you received for question (25), calculate the equilibrium constant for the reaction. Use ΔG = -RT ln K: Temperature 25 Celsius, R = 8.314 J / mol. K

HCl, HBr and HI are strong acids; however, HF is a weak acid. What is the best explanation for this phenomenon?

Embalming practices do not vary from country to country so viewing is rarely a problem when human remains are received from other countries.

What is the concentration of the ions in 3.0 L of 1.0 MAl2(CO3)3?   Answer       [Al 3+]          [CO 3 2 -]      A 0.33 M 0.50 M B 0.66 M 0.99 M C 2.0 M 3.0 M D 3.0 M 4.5 M

Calculate the Ecell for the following reaction? Zn(s)  +  Fe2+(aq, 0.1 M)  ↔  Zn2+(aq, 1.9 M)  +  Fe(s) Use:  Zn2+(aq)  +  2e-  ↔  Zn(s)  Ecell = -0.76 V Fe2+(aq)  = 2e-  ↔  Fe(s)  Ecell = -0.447 V

Predict the products for the following reaction Zn(s)  +  2H+(aq)   →   

Acidity of H-halogen is increasing down the group. Which of the following statement best describes this phenomenon?

Based on the answer you received for question 23, determine whether the cell is spontaneous or non-spontaneous Pb2+(aq)  +  2e-  = Pb(s)       Ecell = -0.13 V Ca2+(aq)  +  2e-  = Ca(s)     Ecell= -2.87 V Choose (A) or (B)

During a redox reaction