CHEM1011-CHEM1031-CHEM1051-Chemistry 1A (T1 2025)
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Which transformation could take place at the anode of an electrochemical cell?
Balance the following equation for the reaction under acidic aqueous conditions.
Fe2+ + Cr2O72– → Fe3+ + Cr3+
What will the coefficient for water in the balanced reaction be?
The oxidation state of titanium in TiO is _____.
Which transformation would you expect to take place at the cathode of an electrochemical cell?
Balance the following oxidation-reduction reaction using the half-reaction method for the reaction under acidic aqueous conditions.
Cr2O72– + I2→ Cr3+ + IO3–
In the balanced equation, what is the coefficient of water?
The oxidation state of chlorine in Cl2 is
Consider the following statements:
| (i) | A reduction half equation contains at least one species that is being reduced and at least one electron on the left hand side of the reaction arrow. |
| (ii) | A redox reaction in an electrochemical cell involves electron transfer between two species where electrons travel between two electrodes via an external electrical circuit. |
| (iii) | A redox reaction where all species are in direct contact with one another does not involve electron transfer. |
The reaction below is exothermic:
2SO2 (g) + O2 (g) ⇌ 2SO3 (g)Le Châtelier's Principle predicts that ________ will result in an increase in the number of moles of SO3 (g) in the reaction container.
Consider the reaction below, for which K = 7.26 × 10–2 at 450.0 °C.
2Cl2 (g) + 2H2O (g) ⇌ 4HCl (g) + O2 (g)What is the value of K at this temperature for the following reaction? Cl2 (g) + H2O (g) ⇌ 2HCl (g) + ½O2 (g)
Consider the following equilibrium reaction:
H2CO3 (aq) ⇌ H+ (aq) + HCO3– (aq); K = 5.0 x 10–7
If the initial concentrations of the species are:
[H2CO3] = 0.12 M; [H+] = 5.00 x 10–5 M; [HCO3–] = 4.00 x 10–3 M
Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?
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