Q1) chemist has to titrate an acid with a molecular formula containing only carbon, hydrogen, and oxygen with the respective percentages: 53.66% (C), 4.09% (H) and 42.25% (O) by mass. To reach the equivalence point the chemist used 18.02 mL of NaOH solution 0.0406 (M) to neutralize 0.3602 g of this acid. Assuming that the acid is monoprotic (there is only one acidic hydrogen per molecule of acid): 1. Calculate the number of mole of acid used in the titration. 2. What is the empirical formula of the acid? 3. What is the molecular formula of the acid?
Q2) In an experiment 26.0 g of powdered iron (III) oxide is mixed with 3g carbon and heated to 500°C in a rigid 6.0 L reactor. The following reaction occurred:
Assume that the reaction is 100% complete, the volume of Fe(s) and C(s) is small enough to be ignored, and the temperature of the reactor is maintained at 500 °C.
Write the balanced reaction.
Calculate the number of moles of gas formed.
What will be the pressure of the gas in the reactor after the reaction?
of powdered iron (III) oxide is mixed with 
carbon and heated to 
in a rigid 
reactor.
complete, the volume of Fe(s) and C(s) is small enough to be ignored, and the temperature of the reactor is maintained at 
