CEM 141 Study Guide - Midterm Guide: Boiling Point, Orbital Hybridisation, Isoelectronicity

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Learning goals for cem 141 exam 2 (stoichiometry, chapter 2 and chapter 3) Learning goals for stoichiometry: (not in text use web materials) X, uv, visible, ir, radio: describe and identify experimental evidence for why light is a wave (diffraction, interference, make an argument (claim, evidence and reasoning) about why we can consider electromagnetic radiation as a wave. Big idea 5: atomic theories change over time as new experimental evidence is produced: describe how the model of the atom changed from dalton through thompson, Explain why each model changed and point out the problems with the previous model: choose an atomic model to explain a phenomenon, and explain why you chose that model. Learning goals and big ideas for chapter 3. The macroscopic properties of a substance can be explained by the interactions at the molecular level. We can explain bonding using a number of different models (e. g. valence bond, molecular orbital, metallic)

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To understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. Stoichiometry describes the quantitative relationships among the reactants and products of a balanced reaction by directly comparing mole ratios. Stoichiometry can be used to convert mass, number of moles, or number of partides between products and reactants, as shown in the flowchart displayed in the figure. (Figure 1) How many grams of NH3 can be produced from 2.21molofN2 and excess HÂ« Express your answer numerically in grams. How many grams of H2 3re needed to produce 10.14g of NH3 ? Express your answer numerically in grams. How many molecules {not moles) of NHa are produced from 8.42 times 10-1g of Hg? Express your answer numerically as the number of molecules. In the following chemical reaction 2 mol of A will react with 1 mol of B to produce 1 mol of A B without anything left over: But what if you re given 2.8 mol of A and 3.2 mol of B7 The amount of product formed is limited by the reactant that runs out first, called the limiting reactant. To identify the limiting reactant, calculate the amount of product formed from each amount of reactant separately: Notice that less product is formed with the given amount of reactant A. Thus. A is the limiting reactant, and a maximum of 1.4 mol of A2B can be formed from the given amounts. If you had excess chlorine, how many moles of of aluminum chloride could be produced from 11 .Og of aluminum'7 Express your answer to three significant figures and include the appropriate units. Part B If you had excess aluminum, how many moles of aluminum chloride could be produced from 16.0g of chlorine gas, Limiting Reactant Procedure Express your answer to three significant figures and include the appropriate units. Part C Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: What is the maximum mass of aluminum chloride that can be formed when reacting 11.0g of aluminum with 16.3g of chlorine17 Express your answer to three significant figures and include the appropriate units.

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?

CEM 141 Study Guide - Midterm Guide: Boiling Point, Orbital Hybridisation, Isoelectronicity

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