Aqa chemistry paper 2

• Equilibrium of a redox reaction can be changed by altering the concentrations of reactants or products.
• The equation for the reaction between hydrochloric acid and magnesium is Mg + 2HCl → MgCl2 + H2
• Oxidation involves the loss of electrons and reduction involves the gain of electrons.
• Oxidation involves the loss of electrons and reduction involves the gain of electrons.
• Redox reactions involve the transfer of electrons between oxidizing and reducing agents.
• Redox reactions involve the transfer of electrons between oxidizing and reducing agents.
• The equation for the reaction between sodium carbonate and sulfuric acid is Na2CO3 + H2SO4 → Na2SO4 + CO2 + H2O
• The equation for the reaction between copper oxide and dilute nitric acid is CuO + 2HNO3 → NO2 + H2O + Cu(NO3)2
• The equation for the reaction between iron filings and dilute hydrochloric acid is Fe + 2HCl → FeCl2 + H2
• The equation for the reaction between iron filings and dilute hydrochloric acid is Fe + 2HCl → FeCl2 + H2
• The equation for the reaction between iron filings and dilute hydrochloric acid is Fe + 2HCl → FeCl2 + H2
• The equation for the reaction between copper metal and silver nitrate solution is Cu + 2AgNO3 → Ag2Cu(NO3)2
• A redox reaction occurs when one substance loses electrons while another gains them.
• In an electrolysis cell, the cathode is negatively charged and attracts positive ions (cations) from the solution to form metal atoms at the surface of the cathode.
• In an electrolysis cell, the cathode is negatively charged and attracts positive ions (cations) from the solution to form metal atoms at the surface of the cathode.
• An example of a redox reaction is the rusting of iron, where Fe(s) reacts with oxygen gas (O2) to produce ferric oxide (Fe2O3).
• An example of a redox reaction is the rusting of iron, where Fe(s) reacts with oxygen gas (O2) to produce ferric oxide (Fe2O3).
• In an electrolysis cell, the cathode is negatively charged and attracts positively charged metal ions from the solution to form metal atoms on its surface.
• In an electrolysis cell, the positive terminal is called the anode and the negative terminal is called the cathode.
• In an electrolysis cell, the positive terminal is called the anode and the negative terminal is called the cathode.
• Acids release hydrogen ions when they dissolve in water, while bases accept hydrogen ions from other compounds.
• Acids release hydrogen ions when they dissolve in water, while bases accept hydrogen ions from other compounds.
• Aqueous solutions are used to dissolve substances that do not readily dissolve in water, such as sodium chloride (NaCl) and potassium iodide (KI).
• Aqueous solutions are used to dissolve substances that do not readily dissolve in water, such as sodium chloride (NaCl) and potassium iodide (KI).
• Reduction reactions involve the gain of electrons and oxidation reactions involve the loss of electrons.
• Reduction reactions involve the gain of electrons and oxidation reactions involve the loss of electrons.
• The equation for the reaction between aluminum metal and dilute hydrochloric acid is Al + 6HCl → AlCl3 + 3H2
• The equation for the reaction between aluminum metal and dilute hydrochloric acid is Al + 6HCl → AlCl3 + 3H2
• The equation for the reaction between iron filings and hydrochloric acid is Fe + 2HCl → Cl2 + FeCl2
• The equation for the reaction between iron filings and hydrochloric acid is Fe + 2HCl → Cl2 + FeCl2
• The equation for the reaction between magnesium ribbon and dilute hydrochloric acid is Mg + 2HCl → MgCl2 + H2