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
- A 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_forwardOne 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_forward99 Pure gaseous nitrogen dioxide (NO2) cannot be obtained, because NO2dimerizes, or combines with itself, to produce a mixture of NO2 and N2O4. A particular mixture of NO2, and N2O4 has a density of 2.39 g/L at 50°C and 745 torr. What is the partial pressure of NO2 in this mixture?arrow_forward
- The oxides of Group 2A metals (symbolized by M here) react with carbon dioxide according to the following reaction: MO(s)+CO2(g)MCO3(s) A 2.85-g sample containing only MgO and CuO is placed in a 3.00-L container. The container is filled with CO2 to a pressure of 740. torr at 20.C. After the reaction has gone to completion, the pressure inside the flask is 390. torr at 20.C. What is the mass percent of MgO in the mixture? Assume that only the MgO reacts with CO2.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_forwardWhen acetylene, C2H2, is burned in oxygen, carbon dioxide and steam are formed. A sample of acetylene with a volume of 7.50 L and a pressure of 1.00 atm is burned in excess oxygen at 225C. The products are transferred without loss to a 10.0-L. flask at the same temperature. (a) Write a balanced equation for the reaction. (b) What is the total pressure of the products in the 10.0-L flask? (c) What is the partial pressure of each of the products in the flask?arrow_forward
- A 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_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_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_forward
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