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When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) (a) What is the theoretical yield of Li3N in grams when 12.7 g of Li is heated with 34.7 gof N2? (b) If the actual yield of Li3N is 5.45 g, what is the percent yield of the reaction?
(a) 21.2 g (b) 25.7 %
Balance the following equations. Do not include the states of matter. (a) C + O2 → CO (b) KOH + H3PO4 → K3PO4 + H2O (c) N2 + H2 → NH3 (d) K + H2O → KOH + H2
(a) 2C + O2 → 2CO (b) 3KOH + H3PO4 → K3PO4 + 3H2O (c) N2 + 3H2 → 2NH3 (d) 2K + 2H2O → 2KOH + H2
Nitroglycerin (C3H5N3O9) is a powerful explosive. Its decomposition may be represented by 4C3H5N3O9 → 6N2 + 12CO2 + 10H2O + O2 This reaction generates a large amount of heat and gaseous products. It is the sudden formation of these gases, together with their rapid expansion, that produces the explosion. (a) What is the maximum amount of O2 in grams that can be obtained from 2.50 × 10^2 g of nitroglycerin? (b) Calculate the percent yield in this reaction if the amount of O2 generated is found to be 8.20 g
(a) 8.81 g (b) 93.1 %
Industrially, hydrogen gas can be prepared by combining propane gas (C3H8) with steam at about 400°C. The products are carbon monoxide gas (CO) and hydrogen gas (H2). (a) Write a balanced equation for the reaction. (b) How many kilograms of H2 can be obtained from 4.35 × 10^3 kg of propane? ____× 10^____ kg H2 gas
(a) C3H8(g) + 3H2O(g) → 3CO(g) + 7H2(g) (b) 1.39201026 × 10^3 kg H2 gas
Write an unbalanced equation to represent each of the following reactions: Do not include phase abbreviations. (a) Nitrogen and oxygen react to form nitrogen dioxide. (b) Dinitrogen pentoxide reacts to form dinitrogen tetroxide and oxygen. (c) Ozone reacts to form oxygen. (d) Chlorine and sodium iodide react to form iodine and sodium chloride. (e) Magnesium and oxygen react to form magnesium oxide.
(a) N₂ + O₂ → NO₂ (b) N₂O₅ → N₂O₄ + O₂ (c) O₃ → O₂ (d) Cl₂ + NaI → I₂ +NaCl (e) Mg + O₂ → MgO
Tetraphosphorous decoxide (P4O10) reacts with water to produce phosphoric acid. (a) Write the balanced equation for this reaction. Do not include states of matter in the equation. (b) Determine the number of moles of P4O10 required to produce 6.00 moles of phosphoric acid. (c) Determine the number of moles of water required to produce 6.00 moles of phosphoric acid.
(a) P₄O₁₀ + 6H₂O → 4H3PO4 (b) 1.50 mol (c) 9 mol
Determine whether each of the following equations represents a combination reaction, a decomposition reaction, or a combustion reaction: (a) 2NaHCO3 → Na2CO3 + CO2 + H2O (b) NH3 + HCl → NH4Cl (c) 2CH3OH + 3O2 → 2CO2 + 4H2O
(a) decomposition reaction (b) combination reaction (c) combustion reaction
What is the maximum mass, in grams, of P2I4 that can be prepared from 7.23 g of P4O6 and 11.20 g of iodine according to the reaction: 5P4O6 + 8I2 → 4P2I4 + 3P4O10
12.5 g P2I4
The interhalogen compound ClF3 reacts with NH3 to produce three products according to the figure shown If 28.4 g of NH3 and 167.3 g of ClF3 are allowed to react, what masses of each product would be recovered assuming complete reaction? ____g N2 ____g Cl2 ____g HF
23.4 g N2 59.1 g Cl2 100 g HF
Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation: N2(g) + 3H2(g) → 2NH3(g) Calculate the mass of ammonia produced when 20.0 g of nitrogen react with 14.8 g of hydrogen. ____ g NH3 Which is the excess reactant and how much of it will be left over when the reaction is complete: hydrogen or nitrogen ____g
24.31750519 g NH3 Hydrogen 10.48249661 g excess H2
Which of the following equations best represents the reaction shown in the diagram
2A + B → C + D
Write and balance the equation for the combination of ammonia gas with solid copper(II) oxide to produce copper metal, nitrogen gas, and liquid water. Include the states of matter.
2NH3(g) + 3CuO(s) → 3Cu(s) + N2(g) + 3H2O(l)
The fertilizer ammonium sulfate, (NH4)2SO4, is prepared by the reaction between ammonia (NH3) and sulfuric acid: 2NH3(g) + H2SO4(aq) → (NH4)2SO4(aq) How many kilograms of NH3 are needed to produce 1.30 × 10^5 kg of (NH4)2SO4? Enter your answer in scientific notation
3.35093901 × 10^4 kg
Consider the combustion of carbon monoxide (CO) in oxygen gas: 2CO(g) + O2(g) → 2CO2(g) Starting with 3.46 moles of CO, calculate the number of moles of CO2 produced if there is enough oxygen gas to react with all the CO.
3.46 mol CO2
Fermentation is a complex chemical process of wine making in which glucose is converted into ethanol and carbon dioxide: C6H12O6 → 2C2H5OH + 2CO2 glucose ethanol Starting with 827.6 g of glucose, what is the maximum amount of ethanol in grams and in liters that can be obtained by this process (density of ethanol = 0.789 g/mL)?
423.2572803 g 0.536447757 L
Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction: CaF2 + H2SO4 → CaSO4 + 2HF In one process, 6.15 kg of CaF2 is treated with an excess of H2SO4 and yields 2.45 kg of HF. Calculate the percent yield of HF.
77.7 % yield
Menthol is a flavoring agent extracted from peppermint oil. It contains C, H, and O. In one combustion analysis, 10.00 mg of the substance yields 11.53 mg H2O and 28.16 mg CO2. What is the empirical formula of menthol? Add subscripts to complete the empirical formula. CHO
C10H20O
Write and balance the chemical equation that represents the reaction of aqueous sulfuric acid with aqueous sodium hydroxide to form water and sodium sulfate. Include phases.
H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l)
Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas: 2NO(g) + O2(g) → 2NO2(g) In one experiment, 0.893 mol of NO is mixed with 0.519 mol of O2. Determine which of the two reactants is the limiting reactant. Calculate also the number of moles of NO2 produced.
Limiting reactant: NO Moles of NO2 produced: 0.893 mol
Consider the reaction 2A + B → C In the diagram here that represents the reaction, which reactant, A or B, is the limiting reactant?
The limiting reactant = A
Ammonia is a colorless gas with a pungent, characteristic odor. It is prepared by the reaction between hydrogen and nitrogen: 3H2(g) + N2(g) → 2NH3(g) In a particular reaction, 9.3 moles of NH3 were produced. How many moles of H2 and how many moles of N2 were consumed to produce this amount of NH3?
moles H2 = 13.95 moles N2 = 4.65
Nitrogen and hydrogen react to form ammonia according to the following balanced equation: N2(g) + 3H2(g) → 2NH3(g) Calculate the number of moles of hydrogen required to react with 0.0747 mole of nitrogen, and the number of moles of ammonia that will form. moles of hydrogen = ____mol moles of ammonia = ____mol
moles of hydrogen = 0.2241 mol moles of ammonia = 0.1494 mol
