CHEM 6B Lecture Notes - Lecture 1: Molar Mass, Empirical Formula, Royal Aircraft Factory F.E.2

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burgundyporpoise729

6 Apr 2018

School

UCSD

Department

Chemistry and Biochemistry

Course

CHEM 6B

Professor

Sandrine Bernoilles

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Document Summary

Fe(no3)3: mass % = (part / whole) x 100% = mass fe / mass molar, 1 fe, 3 n, 9 o (55. 485) / (55. 485 + 3*14. 0067 + 9*15. 9994) = 0. 2298 x 100% = C4h5n2o: phosphorous reacts with oxygen to produce a specific oxide. This oxide is formed in the lab when you react 1. 347g of phosphorous and 1. 744g of oxygen. What is the empirical formula: 0. 04348863 mol p, 0. 10900681, divide both by smaller number (0. 04348863, 1:2. 5 = 2:5, empirical formula: p2o5. 44518: 9. 37g h2o * (2*1. 00794/18. 01528) = 1. 048g h / 1. 00794. 0. 24250 mol c: 4. 40g h2o * (2*1. 00794/18. 01528) = 0. 4924g h / 1. 00794 = 0. 4885 mol h: 4. 40 - 2. 9126 - 0. 4924 = 0. 995g o / 15. 994 = 0. 06221mol. If 2. 72 moles of iron are reacted with excess oxygen, how many moles of iron (iii) oxide will be formed: 4fe + 3o2 -> 2fe2o3, dimensional analysis: 2. 72 mol fe 2 mol fe2o3 = 1. 36 moles.

Related Questions

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?

CHEM 6B Lecture Notes - Lecture 1: Molar Mass, Empirical Formula, Royal Aircraft Factory F.E.2

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