CHEM1011 Lecture Notes - Lecture 1: Tantalum, Kilogram, Ideal Gas Law

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2 nomenclature of simple organic and inorganic ions. 1 name the constituent parts of an atom, together with their relative masses and charges. 2 calculate numbers of protons, neutrons, electrons in atoms of a particular element. 3 name simple inorganic compounds and write the formulae for simple compounds from their name. 5 calculate % by mass of each element in a compound and determine empirical formula from % by mass. 6 calculate concentration of solutions in various units. Calculate yield in a chemical reaction, determine the limiting reagent. It is the science concerned with the composition, structure, properties of matter, as well as changes it undergoes during chemical reactions. Chem : study of matter , matter= anything that takes up spaces and has mass. Matter can be mixtures / pure substances-> pure substances could be either elements / compounds. De(cid:373)o(cid:272)(cid:396)itus: (cid:862)the(cid:396)e (cid:271)e ato(cid:373)s a(cid:374)d the(cid:396)e (cid:271)e (cid:448)oid. (cid:863) Dalton: first atomic theory supported with observation and measurement.

Related Questions

A certain compound has the following elemental analysis (percent composition by mass), where âXâ is an unknown element (N, O, Cl, or Br):

% C 74.93; % H 12.59; % X 12.48

Its IR spectrum and mass spectrum are given below. Answer the questions on the next page. While you do not need to fully analyze all of this data or determine the exact structure, you may wish to use different spectral details to help determine certain functional groups or other substructures.

a. What element is element X? Explain your reasoning briefly.

b. Calculate the empirical formula of this compound. Remember to

include all your work.

c. Write the mass of the molecular ion (M+ signal of mass spectrum).

d. Calculate the molecular formula of the compound.

e. Write the mass of the base peak as seen on the mass spectrum

f.â What structural fragment(s) were lost from the molecular ion to give the peak whose relative intensity is approximately 70 on the mass spectrum? You may wish to figure out a subset of the molecular formula itself that represents the lost mass, and then figure out some simple alkyl(s) or other group(s) that could give that total formula.

CHM111

Q1. Which of the following contains the MOST atoms? You shouldn't need to do a calculation here.

A) 10.0 g Ne

B) 10.0 g He

C) 10.0 g Ar

D) 10.0 g Kr

E) 10.0 g Mg

Q2. How many atoms are present in 0.23 moles of Calcium?

Q3. How many atoms are present in 5.6 mg of Silicon?

Q4. How many grams of iodine do 5.6 x 10²⁵ atoms of iodine represent?

Q5. Balance the following Chemical Equations:

_____ CaC₂(s) + _____H₂O(l) ? _____ Ca(OH)₂(aq) + _____ C₂H₂(g)

_____ P₄O₁₀ + _____ H₂O? ______ H₃PO₄

___ C₃H₈O₃ + ___ O₂ ? ___ CO₂ + ___ H₂O

_____ C₄H₁₀(l) + _____ O₂(g) ? _____ CO₂(g) + _____ H₂O(g)

___ Al + ___ N₂ ? ___ Al₂N₃

___ NaN₃ ? ___ Na + ___ N₂

___ C₃H₅N₃O₉ ? ___ CO₂ + ___ N₂ + ___ H₂O + ___ O₂

Q6. Calculate the percent composition of each element in Al(NO₃)₃

Q7. A 65.0 g sample of a pure compound containing only Nickel, Oxygen and Carbon is found to contain 22.36 g Nickel and 18.27 g Carbon. What is the empirical formula of compound?

Q8. Determine the Empirical formula and Molecular formula of a compound that contains: 65.4% C, 9.15% H and 25.4% N by mass and has a molar mass of 220 g/mol.

Q9. Oxygen gas can be produced by the decomposition of KClO₃

2KClO₃ (s) ? 2 KCl + 3 O₂ (g)

How many grams of O₂ can be produced from 1.625 g of KClO₃?

Q10. Consider the following balanced reaction: 2 Fe (s) + Al₂O₃ (s) Â® 2 Al (s) + Fe₂O₃ (s)

If 6.25 moles of Fe react with 2.50 moles of Al₂O₃

Which reactant is the limiting reagent?

How many grams of Al are produced?

Q11. Consider the reaction for the manufacture of Aluminum sulfate:

2 AlCl₃ (aq) + 3 H₂SO₄ (aq) ? Al₂(SO₄)₃(aq) + 6 HCl (aq)

If 15.0 g of AlCl₃was mixed with 25.0 g of H₂SO₄, which reactant is the limiting reagent?

Calculate the theoretical yield of Al₂(SO₄)₃.

If only 18.63 g of Al₂(SO₄)₃ was produced, what is the percent yield of Al₂(SO₄)₃?

Q13. How many grams of Nickel (II) chloride are needed to prepare 100.0 ml of 0.125 M solution?

Q14. What volume of 0.125 M KMnO₄ (aq) solution can be prepared from 12.623 g of KMnO₄?

CHEM1011 Lecture Notes - Lecture 1: Tantalum, Kilogram, Ideal Gas Law

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