Calculations quiz Loading... 1. State the steps for calculating empirical formula1) Aᵣ/mass. 2) divide by the smallest. 3) Give the ratio has a whole number. 4) State final empirial formula1) mass/Aᵣ. 2) divide by the largest. 3) Give the ratio has a whole number. 4) State final empirial formula1) Aᵣ/mass. 2) divide by the largest. 3) Give the ratio has a whole number. 4) State final empirial formula1) mass/Ar. 2) divide by the smallest. 3) Give the ratio has a whole number. 4) State final empirial formulaQuestion 1 of 9 Loading... 2. How many protons in a phosphorus atom?31151216Question 2 of 9 Loading... 3. Which particle(s) in an atom has the smallest mass?Electrons and neutronsProtonNeutronElectronQuestion 3 of 9 Loading... 4. What is meant by the term molecular formula?A method of calculating the mass needed to make a certain yield in an equationA chemical formula that shows the actual numbers of the different types of atoms in a moleculeA method of calculating the ratios of masses in an equationA chemical formula that shows the simplest ratio of the numbers of atoms in a compoundQuestion 4 of 9 Loading... 5. To determine the formula of a metal oxide by combustion, magnesium is heated in a crucible. Why is the crucible is cooled, weighed, reheated, cooled, re-weighed, and so on?To make sure the mass is still going down so the magnesium is still reactingTo make sure a constant mass has been reached and there is no more magnesium left to reactTo ensure all the magnesium oxide to escapeTo allow any water to escapeQuestion 5 of 9 Loading... 6. How many electrons can the first shell hold?210818Question 6 of 9 Loading... 7. A compound that contained 24.24% Carbon. 4.04% Hydrogen and 71.72% Chlorine and has a relative molecular mass of 99. Calculate the empirical formula and the molecular formula.Empirical formula is C₂H₄Cl₂. Molecular formula is CH₂ClEmpirical formula is CH₂Cl. Molecular formula is C₂H₄Cl₂Empirical formula is C₂H₄Cl₂. Molecular formula is C₂H₄Cl₂Empirical formula is CH₂Cl. Molecular formula is CH₂ClQuestion 7 of 9 Loading... 8. A sample of bromine contained the two isotopes in the following proportions: bromine-79 = 50.7% and bromine-81 = 49.3%. Calculate the relative atomic mass of bromine((81x50.7)+(79x49.3))/100 = 80.01(81 + 79)/2 = 80(81x79)/100 = 63.99((79x50.7)+(81x49.3))/100 = 79.99Question 8 of 9 Loading... 9. Calculate the relative formula mass(Mr) of aluminium nitrate (Al(NO₃)₃)89213185117Question 9 of 9 Loading... Related Posts:The entire quiz question bank!The entire quiz question bank (Double only)!Key Calculations quizEquilibria (triple) quizCondensation Polymers quizElectrolysis quiz Hydr0Gen2020-02-16T16:38:53+00:00Categories: Uncategorized|Tags: Quiz, Topic: Calculations| Share This Story, Choose Your Platform! FacebookXRedditLinkedInTumblrPinterestVkEmail
