Starting with the same mass of the following four solids, and the other reactant HCl(aq) being always in excess, which of the following would show the correct increasing order of the calculated ngas (either H2 or co2), assuming all other parameters are held constant? Mg(s) [MW = 55.85 g/mol] Ag(s) [MW = 107.8682 g/mol] NaHCO3(s) [MW = 84.007 g/mol] CaCO3(s) [MW = 100.0869 g/mol] %3D %3D %3D O a. Mg < CaCO3 < NaHCO3 < Ag O b. Ag < CaCO3 < NaHCO3 < Mg O c. Mg < Ag < NaHCO3 < CACO3 O d. Ag < Fe < NaHCO3 < CaCO3

Starting with the same mass of the following four solids, and the other reactant HCl(aq) being always in excess, which of the following would show the correct increasing order of the calculated ngas (either H2 or co2), assuming all other parameters are held constant? Mg(s) [MW = 55.85 g/mol] Ag(s) [MW = 107.8682 g/mol] NaHCO3(s) [MW = 84.007 g/mol] CaCO3(s) [MW = 100.0869 g/mol] %3D %3D %3D O a. Mg < CaCO3 < NaHCO3 < Ag O b. Ag < CaCO3 < NaHCO3 < Mg O c. Mg < Ag < NaHCO3 < CACO3 O d. Ag < Fe < NaHCO3 < CaCO3

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 63QAP: Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L....

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105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)
Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)
Consider the following reaction at 75C: 3R(s)+2Q(g)A(g)+5B(l)K=9.4 A 10.0-L sample contains 0.30 mol of R and Q and 0.50 mol of A and B. In which direction will the reaction proceed?
Methanol (CH3OH) can be produced by the following reaction: CO(g)+2H2(g)CH3OH(g) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g methanol is produced per minute, what is the percent yield of the reaction?
Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25C. The reaction vessel is heated to 400C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of F2 at 25C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?
At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22C the vapor pressure of water is 19.8 torr.)
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
Ammonium perchlorate (NH4ClO4) is a solid rocket fuel that was used in space shuttles. When heated at 200oC, it decomposes to a variety of gases, with the most important being N2(g), Cl2(g), O2(g), and H2O (g). Write a balanced chemical equation for the decomposition of NH4ClO4, assuming that only the products listed above are generated. The sudden appearance of hot gaseous products in a small initial volume leads to a rapid increase in pressure and temperature, which give the rockets its thrust. What total pressure of gas would be produced at 800 oC by igniting 7.00x105 kg of NH4ClO4 and allowing it to expand to a volume of 6.4x106L? (assume ideal gas behavior). Calculate the molar fraction of Cl2 and its partial pressure.
Consider the reaction of a mixture of NaHCO3 and Ca(HCO3)2 with excess HCl. The net ionic reaction observed is H+(aq) + HCO3-(aq) → H2O(l) + CO2(g) The data for this problem is for 25 oC The above sample of gas (15.2 L, STP) contains 0.447 mol of N2. What is the mole fraction of nitrogen in that sample of gas? X = ___

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