Concept explainers
56 Consider the following reaction:
What mass of NiO will react with a sample of ClF3 ags that has a pressure of 250 torr in a 2.5-L flask at
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Chapter 5 Solutions
Chemistry for Engineering Students
- 52 If tetraborane, B4H10, is treated with pure oxygen, it burns to give B2O3 and H2O: 2B4H10(s)+11O2(g)4B2O3(s)+10H2O(g) If a 0.050-g sample of tetraborane burns completely in O2, what will be the pressure of the gaseous water in a 4.25-L flask at 30.0 C?arrow_forwardAmmonia gas is synthesized by combining hydrogen and nitrogen: 3 H2(g) + N2(g) 2 NH3(g) (a) If you want to produce 562 g of NH3, what volume of H2 gas, at 56 C and 745 mm Hg, is required? (b) Nitrogen for this reaction will be obtained from air. What volume of air, measured at 29 C and 745 mm Hg pressure, will be required to provide the nitrogen needed to produce 562 g of NH3? Assume the sample of air contains 78.1 mole % N2.arrow_forwardA chemist weighed out 5.14 g of a mixture containing unknown amounts of BaO(s) and CaO(s) and placed the sample in a 1.50-L flask containing CO2(g) at 30.0C and 750. torr. After the reaction to form BaCO3(s) and CaCO3(s) was completed, the pressure of CO2(g) remaining was 230. torr. Calculate the mass percentages of CaO(s) and BaO(s) in the mixture.arrow_forward
- One way to synthesize diborane, B2H6, is the reaction 2 NaBH4(s) + 2 H3PO4() B2H6(g) + 2 NaH2PO4(s) + 2 H2(g) (a) If you have 0.136 g of NaBH4 and excess H3PO4, and you collect the resulting B2H6 in a 2.75-L flask at 25 C, what is the pressure of the B2H6 in the flask? (b) A by-product of the reaction is H2 gas. If both B2H6 and H2 gas come from this reaction, what is the total pressure in the 2.75-L flask (after reaction of 0.136 g of NaBH4 with excess H3PO4) at 25 C?arrow_forwardNitrogen trifluoride is prepared by the reaction of ammonia and fluorine. 4 NH3(g) + 3 F2(g) 3 NH4F(s) + NF3(g) If you mix NH3 with F2 in the correct stoichiometric ratio, and if the total pressure of the mixture is 120 mm Hg, what are the partial pressures of NH3 and F2? When the reactants have been completely consumed, what is the total pressure in the flask? (Assume T is constant.)arrow_forwardA mixture contained calcium carbonate, CaCO3, and magnesium carbonate, MgCO3. A sample of this mixture weighing 7.85 g was reacted with excess hydrochloric acid. The reactions are CaCO3(g)+2HCL(aq)CaCl2(aq)+H2O(I)+CO2(g)MgCO3(s)+2HCL(aq)MgCl2(aq)+H2O(I)+CO2(g) If the sample reacted completely and produced 1.94 L of carbon dioxide, CO2, at 25C and 785 mmHg, what were the percentages of CaCO3 and MgCO3 in the mixture?arrow_forward
- A sample of a smoke stack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by each gas?arrow_forwardSulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid. S(s)+O2(g)SO2(g)2SO2(g)+O2(g)2SO3(g) 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?arrow_forwardMagnesium burns in air to produce magnesium oxide, MgO, and magnesium nitride, Mg3N2 Magnesium nitride reacts with water to give ammonia. Mg3N2(s)+6H2O(l)3Mg(OH)2(s)+2NH3(g) What volume of ammonia gas at 24C and 753 mmHg will be produced from 3.93 g of magnesium nitride?arrow_forward
- A mixture contained zinc sulfide, ZnS, and lead sulfide, PbS. A sample of the mixture weighing 6.12 g was reacted with an excess of hydrochloric acid. The reactions are ZnS(s)+2HCL(aq)ZnCl2(aq)+H2S(g)PbS(s)+2HCL(aq)PbCl2(aq)+H2S(g) If the sample reacted completely and produced 1.049 L of hydrogen sulfide, H2S, at 23C and 762 mmHg, what were the percentages of ZnS and PbS in the mixture?arrow_forwardA 1.0-L flask contains 10.0 g each of O2 and CO2 at 25 C. (a) Which gas has the greater partial pressure, O2 or CO2, or are they the same? (b) Which molecules have the greater rms speed, or are they the same? (c) Which molecules have the greater average kinetic energy, or are they the same?arrow_forward47 HCl(g) reacts with ammonia gas, NH3(g), to form solid ammonium chloride. If a sample of ammonia occupying 250 mL at 21 C and a pressure of 140 torr is allowed to react with excess HCl, what mass of NH4Cl will form?arrow_forward
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