Choose the thermodynamic product formed during the reaction depicted below. DBr ABCD OA OD Br A B Br

H2N. Br CI H2N. Br CI H2N. Br CI

Can anyone explain how this reaction happens clearly

Phosphoric and acetic acids are considered to be weak acids; that is, they do not dissociate completely into ions. Were there any differences in reaction rates with magnesium between these two acids? If so, what distinguishing feature of the acids might explain the differences?

Breathalyzers measure the alcohol (ethanol, C2H6O) content in an exhaled breath using a redox reaction. The C2H6O reacts with an acidic solution of potassium dichromate, forming acetic acid. The color of the solution changesbecause some of the orange chromate is converted to the green Cr3+, and the Breathalyzer measures this color change.C2H6O + Cr2O7 = C2H4O2 + Cr3+ (UNBALANCED)(a) Which reactant is oxidized? Which reactant is reduced?Which reactant is the oxidizing agent? Which reactant is the reducing agent?(b) Balance the redox reaction above that occurs in a Breathalyzer. Note the reaction occurs in acidic conditions.(c) What is E° for the reaction if the standard reduction potential for the acetic acid / ethanol half-reaction is 0.058 V?(Note: see Appendix L in the OpenStax textbook for the reduction potential of the other half-reaction)

Complete this table for the reaction T(k) [N2] [H2] [NH3] [Kc] 500 0.115 0.105 0.439   575 0.110   0.128 9.6 At which temperature is the product favored the most?

Predict the product for the following reaction. || excess H₂ Ni, 100 atm, 150°C IV HO V

What is the thermodynamic product of this reaction? HBr Br O Br Br O Br Br Br

Please explain step by step.

Here is a more complex redox reaction involving the dichromate ion in acidic solution: 3S2− + 14H+ + Cr2O72−→ 3S +2Cr3+ + 7H2O Classify each reactant as the reducing agent, oxidizing agent, or neither. (H+, S2-,Cr2O72−)