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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 2F2(g) + Mn(s) → 4 F⁻(aq) + Mn2+(aq)F2(g) + e⁻ → 2 F⁻(aq) E° = +2.87 VMn2+(aq) + 2 e⁻ → Mn(s) E° = -1.18 V

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]

Determine the molar solubility for Ag2C2O4 in pure water. The Ksp for Ag2C2O4 is 3.5 × 10-11.

Determine the identity of the daughter nuclide from the alpha decay of Rn.

What is undergoing reduction in the redox reaction represented by the following cell notation? Cr(s) ∣ Cr3+(aq) ‖ I2(g) ∣ I⁻(aq) ∣ Pt

Describe what changes occur during beta decay.

What is undergoing oxidation in the redox reaction represented by the following cell notation? Mn(s) ∣ Mn2+(aq) ‖ H+(aq) ∣ H2(g) ∣ Pt

Determine the identity of the daughter nuclide from the beta decay of Dy.

How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of  to the equivalence point?

Determine ΔG°rxn for the following reaction at 378 K.CaCO3(s) → CaO(s) + CO2(g)ΔH°= +179.2 kJ; DS°= +160.2 J/K