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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.) Pb(s) + Br2(l) → Pb2+(aq) + 2 Br⁻(aq)Pb2+(aq) + 2 e⁻ → Pb(s) E° = -0.13 VBr2(l) + 2 e⁻ → 2 Br⁻(aq) E° = +1.07 V

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

Determine the rate law and the value of k for the following reaction using the data provided.2 N2O5(g) → 4 NO2(g) + O2(g)[ N2O5]i (M)Initial Rate (M-1s-1)0.093​4.84 × 10-40.084​4.37 × 10-40.224​1.16 × 10-3

In which of the following processes does the substance become more orderly?

Calculate the ΔG° rxn using the following  reaction at 25oC. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔG°rxn = ?  ΔH°f (kJ/mol) -20.6   -296.8 -241.8 S°(J/mol∙K) 205.8 205.2 248.2 188.8

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. 4 F⁻(aq) + Mn2+(aq) → 2F2(g) + Mn(s) F2(g) + 2e⁻ → 2 F⁻(aq) E° = +2.87 VMn2+(aq) + 2 e⁻ → Mn(s) E° = -1.18 V

Calculate ∆S°rxn for the following reaction. The S° for each species is shown below the reaction. 2NO(g) + 2 H2(g) → N2(g) + 2 H2O(l) S°(J/mol∙K)210.8130.7191.669.9

How much energy (in kJ) is evolved during the reaction of [x] g of Fe 2O 3, according to the reaction below?  Assume that there is excess Al. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ   Report your numerical answer as a positive value with the correct number of significant figures and the correct units.

A solution with a hydroxide ion concentration of 4.15 × 10-6 M is ________ and has a hydrogen ion concentration of ________.

Convert the following: [BLANK-1] 1350 mL = ______ L [BLANK-2] 0.6 mg = ______ mcg [BLANK-3] 3.75 g = ______mg [BLANK-4] 57 tsp = ______ mL [BLANK-5] 184 lb = ______ kg (round to tenths place – one decimal) [BLANK-6] 10,425 mcg = _______ g USE ONLY NUMERALS TO ANSWER – NO LABELS