FiltersDone

Question type

Essay

Multiple Choice

Short Answer

True False

Matching

Exam 3: Stoichiometry of Formulas and Equations

Show Answer

Share

---

All types

Filters

Study FlashcardsPractice ExamLearn

Question 31

Multiple Choice

Review LaterAdd Note

Review Later

Calculate the molar mass of tetraphosphorus decaoxide,P₄O₁₀,a corrosive substance which can be used as a drying agent.

A) 469.73 g/mol
B) 283.89 g/mol
C) 190.97 g/mol
D) 139.88 g/mol
E) 94.97 g/mol

F) A) and B)
G) None of the above

Correct Answer

verified

Show Answer

Question 32

Multiple Choice

Review LaterAdd Note

Review Later

Hydroxylamine nitrate contains 29.17 mass % N,4.20 mass % H,and 66.63 mass O.If its molar mass is between 94 and 98 g/mol,what is its molecular formula?

A) NH₂O₅
B) N₂H₄O₄
C) N₃H₃O₃
D) N₄H₈O₂
E) N₂H₂O₄

F) A) and E)
G) All of the above

Correct Answer

verified

Show Answer

Question 33

Multiple Choice

Review LaterAdd Note

Lead(II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography.Calculate the mass of lead in 139 g of Pb(NO₃) ₂.

Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂ and 0.226 g H₂O.If its molar mass is between 158 and 167 g/mol,what is its molecular formula?

The formula CH₃O_0.5 is an example of an empirical formula.

In a correctly balanced equation,the number of reactant molecules must equal the number of product molecules.

You are provided with a 250 mL volumetric flask,deionized water and solid NaOH.How much NaOH should be weighed out in order to make 250.mL of 0.100 M solution?

Aluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when aluminum reacts with oxygen. 4Al(s) + 3O₂(g) $\to$ 2Al₂O₃(s) A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00 g/mol) is allowed to react.What mass of aluminum oxide ( = 101.96 g/mol) can be formed?

For a sample consisting of 2.50 g of methane,CH₄,calculate a.the number of moles of methane present. b.the total number of atoms present.

One mole of methane (CH₄)contains a total of 3 $\times$ 10²⁴ atoms.

Balance the following equation: C₈H₁₈O₃(l) + O₂(g) $\to$ H₂O(g) + CO₂(g)

Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis) . Al(s) + Br₂(l) $\to$ Al₂Br₆(s) [unbalanced] How many moles of Al are needed to form 2.43 mol of Al₂Br₆?

Hydroxylamine nitrate contains 29.17 mass % N,4.20 mass % H,and 66.63 mass % O.Determine its empirical formula.

Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood,pulp and textiles) . SO₂(g) + 2Cl₂(g) $\to$ SOCl₂(g) + Cl₂O(g) If 0.400 mol of Cl₂ reacts with excess SO₂,how many moles of Cl₂O are formed?

Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂ and 0.226 g H₂O.What is its empirical formula?

Calculate the molar mass of Ca(BO₂) ₂·6H₂O.

Calculate the molar mass of (NH₄) ₃AsO₄.

Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron. 3Mg(s) + 2FeCl₃(s) $\to$ 3MgCl₂(s) + 2Fe(s) A mixture of 41.0 g of magnesium ( = 24.31 g/mol) and 175 g of iron(III) chloride ( = 162.2 g/mol) is allowed to react.Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.

One mole of O₂ has a mass of 16.0 g.

Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus.What is its empirical formula?