I got this question as an example question and I have no clue on how to solve part B Chlorine can be produced by the reaction: 2KMnO4 + 16HCl ->2KCl + 2MnCl2 + 5Cl2 + 8H2O (a)What mass of KMnO4 is required to produce 2.5 L of Cl2 gas measured at STP? For part A I got 7.05 g ( 0.044615 moll) (b) Calculate the volume of commercial hydrochloric acid required (Commercial grade hydrochloric acid is 36.0% HCl by weight, and has a density of 1.18 g mL^(–1)).
That is much too low. Please show your calculations. Can you start by figuring what mass of HCl you need?
Indeed. Very strange. I feel ashamed because I didn't follow the rule that I always tell my students: when you get a numerical answer, always try to figure out if the order of magnitude makes sense. I should've checked with the ideal gas law...