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Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

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Question 1

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Hydrogen peroxide decomposes to produce water and oxygen.Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? 2H₂ O₂ (l) $\rightarrow$ 2H₂ O(l) + O₂ (g)

A) 68.0 g $\rightarrow$ 36.0 g + 32.0 g
B) 34.0 g $\rightarrow$ 18.0 g + 16.0 g
C) 90.5 g (\rightarrow\) 47.9 g + 42.6g
D) 2 x g $\rightarrow$ 2 x g + x g
E) y(34.0g) $\rightarrow$ y(18.0g) +(y / 2) (32g)

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Question 2

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Which statement about the following chemical reaction is NOT correct? 3 H₂ (g) + N₂ (g) $\rightarrow$ 2 NH₃ (g)

A) For every two moles of nitrogen consumed, three moles of ammonia are produced.
B) For every mole of nitrogen consumed, two moles of ammonia are produced.
C) For every three moles of hydrogen consumed, two moles of ammonia are produced.
D) For every two moles of ammonia produced, three moles of hydrogen are consumed.
E) Three moles of hydrogen will react with one mole of nitrogen to produce ammonia.

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Question 3

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Fill in the following table regarding the following reaction. $\mathrm{UO}_{2}(s)+4 \mathrm{HF}(a q) \rightarrow \mathrm{UF}_{4}(s)+2 \mathrm{H}_{2} \mathrm{O}(\ell)$

What is the molar mass of sulfuric acid (H₂SO₄) ?

List three reasons why the actual yield for a chemical reaction may differ from the theoretical yield.

What is the difference in the chemistry between photosynthesis and respiration? Show the chemical equations for each.Which one releases energy? Which one stores energy?

Which statement about the following chemical reaction is NOT correct? The molar masses of S₈, O₂, and SO₃ are 256, 32.0, and 80.1 g/mol, respectively. S₈ (s) + 12 O₂ (g) $\rightarrow$ 8 SO₃ (g)

Metallic chromium can be obtained from the mineral chromite (FeCr₂O₄) .What is the mass percent of chromium in chromite?

During fermentation, yeast converts glucose (180.2 g/mol) into ethanol (46.08 g/mol) and carbon dioxide (44.01 g/mol).The unbalanced reaction equation is given below.Balance the equation and find the percent yield for the reaction if 150.0 g of glucose yields 75.0 mL of ethanol (d =0.789 g/mL). C₆ H₁₂ O₆ (aq) $\rightarrow$ C₂ H₅ OH(aq) + CO₂ (g)

Elemental phosphorus (123.88 g/mol) reacts vigorously with halogens at room temperature to produce phosphorus trihalides.What is the theoretical yield in grams) of PF ₃ (87.97 g/mol) when 15.0 g P₄ reacts with 25.0 g F₂ (38.00 g/mol)? P₄ (s) +6 F₂ (g) $\rightarrow$ 4 PF₃ (g)

A gallon of water has a mass of 3.79 kg.How many moles of water is this?

Which statement regarding the carbon cycle is FALSE?

What is the molar mass of phosphorus pentachloride (PCl₅) ?

What mass of nitrogen gas (28.02 g/mol) is produced when 0.500 kg I₂ (253.8 g/mol) is combined with 35.0 g N₂H₄ 32.06 g/mol) ? 2 I₂(s) + N₂H₄ (g) $\rightarrow$ 4 HI(g) + N₂(g)

For which of the following compounds are the empirical and molecular formulas the same? Acetic acid, found in vinegar, CH₃COOH Formaldehyde, used to preserve biological specimens, CH₂O Ethanol, found in beer and wine, CH₃CH₂OH

Without doing any calculations, identify which of the following compounds has the largest percent sodium by mass and which has the smallest.Explain your logic. sodium oxide, Na₂O; sodium hydroxide, NaOH; sodium hydrogen carbonate, NaHCO₃; sodium carbonate, Na₂CO₃; sodium peroxide, Na₂O₂

Gold metal will dissolve in an aqueous sodium cyanide solution in the presence of O₂. Balance the equation showing this process. ____Au(s)+____ NaCN(aq)+ ____O₂ (g)+ ____H₂ O(l) $\rightarrow$ ___NaAu(CN)₂ (aq)+_____ NaOH(aq)

Arizona was the site of a 400,000-acre wildfire in June 2002.How much carbon dioxide was produced by this fire? Assume that the density of carbon on the acreage was 10 kg/m² and that 50% of the biomass burned (10,000 m² = 2.47 acre) .

Diethyl azodicarboxylate, or DEAD, is an explosive compound with the empirical formula C₃H₅NO₂ and a molecular mass of approximately 174 amu.Find its molecular formula.

Which of the following does NOT share the same empirical formula as the others?