What is the empirical formula of a compound with the following composition by mass, 48.0g C, 4.0g H and 48.0g O?
There are 3 Steps to answering this question:But first you need to understand what is meant by empirical formula:The simplest whole number ratio of the atoms of each element present in a compound.1) First work out the number of moles of each element present:Do this by using Moles = Mass(g) / Relative Mass (g/mol) Moles Carbon = 48.0/12 = 4Moles Hydrogen = 4/1 = 4Moles Oxygen = 48/16 = 3 2) Write this number as a ratio and simplify if necessary:4:4:3, cannot be simplified3) Write this ratio as a formula:C4H4O3This is the answer.
EC
Related Chemistry GCSE answers
All answers ▸In fractional distillation the shorter hydrocarbons have lower boiling points and distil off first. Why?
11.25g of hydrated copper (II) sulfate is heated to constant mass. The new mass is found to be 7.19g. What is the formula of the hydrated copper (II) sulfate?
how is steel stronger than iron?
Sodium Hydroxide can react with sulfuric acid in an acid base reaction. Outline the equation for this reaction, name the product. Finally a titration reaction is conducted. Determine the mass of NaOH needed to neutralise 12.4cm^3 of 0.10moldm^-3 H2SO4.