Question 7 if 3L of nitrogen anf 5L of hydrogen were allowed to react, How many liters of NH3(g) could form? Assume all gases are at the same temperature and pressure, and that the limiting reactant is used up. N₂(g) + 3H₂(g). → 2NH3(9)
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- The nitrogen content of organic compounds can be determined by the Dumas method. The compound in question is first reacted by passage over hot CuO(s): CompoundCuO(s)HotN2(g)+CO2(g)+H2O(g) The product gas is then passed through a concentrated solution of KOH to remove the CO2. After passage through the KOH solution, the gas contains N2 and is saturated with water vapor. In a given experiment a 0.253-g sample of a compound produced 31.8 mL N2 saturated with water vapor at 25C and 726 torr. What is the mass percent of nitrogen in the compound? (The vapor pressure of water at 25C is 23.8 torr.)If an electric current is passed through molten sodium chloride, elemental chlorine gas is generated as the sodium chloride is decomposed. :math>2NaCl(1)2Na(s)+Cl2(g) at volume of chlorine gas measured at 767 mm Hg at 25 °C would be generated by complete decomposition of 1.25 g of NaCl?What volume (in liters) of O2, measured at standard temperature and pressure, is required to oxidize 0.400 mol of phosphorus (P4)? P4(s) + 5 O2(g) P4O10(s)
- A student prepares phosphorous acid, H3PO3, by reacting solid phosphorus triiodide with water. PI3(s)+3H2O(l)H3PO3(s)+3HI(g) The student needs to obtain 0.250 L of H3PO3(d=1.651g/cm3). The procedure calls for a 45.0% excess of water and a yield of 75.0%. How much phosphorus triiodide should be weighed out? What volume of water (d=1.651g/cm3) should be used?A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.Nitric acid can be prepared by bubbling dinitrogen pentoxide into water. N2O5(g)+H2O2H+(aq)+2NO3(aq)(a) How many moles of H+ are obtained when 1.50 L of N2O5 at 25C and 1.00 atm pressure is bubbled into water? (b) The solution obtained in (a) after reaction is complete has a volume of 437 mL. What is the molarity of the nitric acid obtained?
- A Boron and hydrogen form an extensive family of compounds, and the diagram below shows how they are related by reaction. The following table gives the weight percent of boron in each of the compounds. Derive the empirical and molecular formulas of compounds A-E.Hydrogen gas is bubbled into a solution of barium hydroxide that has sulfur in it. The equation for the reaction that takes place is H2(g)+S(s)+2OH(aq) S2(aq)+2H2OWhat volume of 0.349 M Ba(OH)2 is required to react completely with 3.00 g of sulfur?Chlorine trifluoride, ClF3, is a valuable reagent because it can be used to convert metal oxides to metal fluorides: 6 NiO(s) + 4 ClF3(g) 6 NiF2(s) + 2 Cl2(g) + 3 O2(g) (a) What mass of NiO will react with ClF3 gas if the gas has a pressure of 250 mm Hg at 20 C in a 2.5-L flask? (b) If the ClF3 described in part (a) is completely consumed, what are the partial pressures of Cl2 and of O2 in the 2.5-L flask at 20 C (in mm Hg)? What is the total pressure in the flask?
- In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric oxide (NO) gas is produced according to the following unbalanced equation: H+(aq)+NO3(aq)+UO2+(aq)NO(g)+UO22+(aq)+H2O(l) If 2.55 102 mL NO(g) is isolated at 29C and 1.5 atm, what amount (moles) of UO2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)Gold is produced electrochemically from an aqueous solution of Au(CN)2 containing an excess of CN. Gold metal and oxygen gas are produced at the electrodes. What amount (moles) of O2 will be produced during the production of 1.00 mole of gold?On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
