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Exercise #1: (4 marks) Balance each of the following redox reactions in acid condition: a) Mg(s) + H2O(g) → Mg(OH)2(s) + H2(8) b) Cr(NO3)3(aq) + Al(s) + Al(NO3)2(aq) + Cr(s) (6 marks) Exercise #2: In both cases write the balanced formula equation of the reaction and then answer to the question. a) If 25.98 mL of 0.1180 M KOH solution reacts with 52.50 mL of CH,COOH solution, what is the molarity of the acid solution? b) If 26.25 mL of 0.1850 M NaOH solution reacts with 25.00 mL of H2SO4, what is the molarity of the acid solution? Exercise # 3: (6 marks) Calculate the pressure exerted by 1.0 mol H2S behaving as (a) a perfect gas, (b) a van der Waals gas when it is confined under the following conditions: (i) at 273.15 K in 22.414 L, (ii) at 500 K in 150 mL. • Given: The van der Waals constants for HS are : a = 4.484 L .atm.mol and b=0.0434 L'mol!. Exercise # 4: (4.5 marks) A vessel of volume 22.4 L contains a mixture of 1.5 mol H2 and 2.5 mol N2 at 273.15 K. Calculate: a) the mole fractions of each component, b) The total pressure of the mixture, c) The partial pressure of each gas. Exercise #5: (4.5 marks) When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write their balanced formula equation, total ionic equation, and net ionic equation: a) Sodium nitrate + Copper(II) sulfate → b) Ammonium bromide + Silver nitrate →
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