Concept explainers
Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid.
What volume of O2(g) at 350.°C and a pressure of 5.25 atm is needed to completely convert 5.00 g sulfur to sulfur trioxide?
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Chapter 8 Solutions
Chemistry: An Atoms First Approach
- 62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?arrow_forwardGive the reaction type: CaCl2•3H2O (s) + ∆ ⟶ CaCl2 (s) + 3H2O (g)arrow_forwardThe Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H₂(g) + N₂ (g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.04 g H₂ is allowed to react with 10.4 g N₂, producing 2.68 g NH3. Part A What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) μÅ Value Units ?arrow_forward
- Consider the Haber process shown below. N2 (g) + 3 H2 (g) → 2 NH3 (g) Which of the following statements IS NOT TRUE? Assume 100% yield. 28 grams of nitrogen gas reacts with 6 grams of hydrogen gas to form 34 grams of ammonia gas. 5 molecules of nitrogen gas reacts with 15 molecules of hydrogen gas to form 10 molecules of ammonia gas. 15 moles of nitrogen gas reacts with 45 moles of hydrogen gas to form 30 moles of ammonia gas. 25 grams of nitrogen gas reacts with 75 grams of hydrogen gas to form 50 grams of ammonia gas.arrow_forwardIn the early days of automobiles, illumination at night was provided by burning acetylene, C2H2. Though no longer used as auto headlamps, acetylene is still used as a source of light by some cave explorers. The acetylene is (was) prepared in the lamp by the reaction of water with calcium carbide, CaC2:CaC2(s) + 2H2 O(l) ⟶ Ca(OH)2(s) + C2 H2(g).Calculate the standard enthalpy of the reaction. The ΔH°f of CaC2 is −15.14 kcal/mol.arrow_forwardPart 1 A student carried out an investigation to observe the effect of changing concentration of sulfuric acid on the breakdown of calcium carbonate (marble) chips. They changed the concentration of the acid between each test but kept the size of the marble chips constant. The full equation for the reaction and a graph of the overall results can be seen below. CaCO3(s) + H₂SO4(aq) → CaSO4(aq) + CO2(g) + H₂O (1) a) b) Rate of Reaction * Concentration of Acid (mol dm³) Explain, using collision theory, why the student obtained these results, and state what they could conclude about the effect of changing concentration of acid on the rate of reaction between calcium carbonate and sulfuric acid. If the student had ground up the calcium carbonate chips into a powder and run the tests again, what would you expect to happen to the rate of reaction? Briefly explain why by applying collision theory. Part 2 The student ran the same experiment, but this time changed the temperature, increasing it…arrow_forward
- Approximately 12 billion kilograms of phosphoric acid (H3PO4) are produced annually for fertilizers, detergents, and agents for water treatment. Phosphoric acid can be prepared by heating the mineral fluoroapatite (Ca5(PO4)3F) with sulphuric acid in the presence of water. Ca5(PO4)3F + 5H2SO4 + 10H20 → 3H3PO4 + 5CaSO4 2H20 + HF If every kilogram of fluoroapatite yields 390 g of phosphoric acid, what is the percent yield? percentarrow_forwardConsider the mixture of Cl2 and F2 in a closed container as illustrated below. What will the contents of the container look like if the molecules undergo the reaction:Cl2(g) + 3 F2(g) → 2 ClF3(g)?arrow_forwardWhat mass, in grams, of C2H2 is needed to form 152.9 g of CO2? Assume excess oxygen. 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g) Consider the following balanced chemical equation: 4KO2(s) + 2H2O(l) → 4KOH(s) + 3O2(g). Determine the mass (in g) of KOH formed if 36.6 g of KO2 reacts with 36.6 g of H2O. Consider the following balanced chemical equation: CS2(g) + 3O2(g) → CO2(g) + 2SO2(g). Determine the mass (in g) of SO2 formed if 196 g of CS2 reacts with 196 g of O2.arrow_forward
- When heated, metal hydroxides decompose to produce a metal oxide and water. Selected the correct balanced equation for the decomposition of calcium hydroxide. CaOH (s) → CaO2 (s) + H2O (g) Ca(OH)2 (s) → CaO (s) + H2O (g) 2 CaOH (s) → 2 CaO (s) + H2O (g) 3 Ca(OH)2 (s) → 3 CaO2 (s) + H2O (g)arrow_forwardThe reaction between ammonia and oxygen is given below: 2 NH3(g) +2 O2(g) → N2O(g) +3 H₂O(1) We therefore know that which of the following reactions can also occur? N2O(g) +3 H2O(l) → 2 NH3(g) +2 O2(g) 4 NH3(g) +5 O2(g) →4 NO(g) + 6 H₂O(g) 4 NO(g) +6 H2O(g) →4 NH3(g) +5 O2(g) None of the Abovearrow_forwardSuppose you are performing a gas-producing reaction to experimentally determine the molar volume of the gas. Mg (s) + 2 HC1 (aq) → MgCl₂ (aq) + H₂ (g) A sample of Mg produces 21.5 mL of H₂ gas. The gas is collected over water at an atmospheric pressure of 769.6 mm Hg at 22 °C, at which the vapor pressure of water is 19.8 mm Hg. What is the experimental value for the molar volume of the hydrogen gas in L/mol?arrow_forward
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