A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into gaseous products. The cylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a 1 atm pressure piston cylinder large insulated water bath. (See sketch at right.) water bath From previous experiments, this chemical reaction is known to release 255. kJ of energy. gases The temperature of the water bath is monitored, and it is determined from this data that 324. kJ of heat flows into the system during the reaction. exothermic Is the reaction exothermic or endothermic? endothermic up ? Does the temperature of the water bath go up or down? down neither in Does the niston nmove in or out? out

A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into gaseous products. The cylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a 1 atm pressure piston cylinder large insulated water bath. (See sketch at right.) water bath From previous experiments, this chemical reaction is known to release 255. kJ of energy. gases The temperature of the water bath is monitored, and it is determined from this data that 324. kJ of heat flows into the system during the reaction. exothermic Is the reaction exothermic or endothermic? endothermic up ? Does the temperature of the water bath go up or down? down neither in Does the niston nmove in or out? out

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Part A Which of the following statements are true? Check all that apply. • View Available Hint(s) There are gas molecules that move slower than the average. The average kinetic energy of gas molecules decreases with decreasing temperature. All the gas molecules in a sample cannot have the same kinetic energy. O The average speed of gas molecules decreases with decreasing temperature. The kinetic energy of a molecule cannot determine its speed. Submit Part B What are each of the following observations an example of? Drag the appropriate items to their respective bins. > View Available Hint(s) 81 F Sunny 90 here to search PrtScn F8 Home F9 End F10 F6 F4 F5 F3
8.) A 1.08 mol sample of Ar gas is confined in a 25.9 liter container at 19.1 °C.If 1.08 mol of Ne gas is added holding the volume and temperature constant, the average kinetic energy of the total system will a. not enough information to answer the question b. remain the same c. increase d. decrease
A sample of chlorine gas has a volume of 0.33 LL at 273 KK and 1 atmatm pressure. What temperature (in ∘C∘C) would be required to increase the volume to 1.2 LL ? Express your answer using three significant figures. What temperature (in ∘C∘C) would be required to decrease the volume to 0.21 LL ? Express your answer using two significant figures.
Space probes to Mars have shown that its atmosphere consists mostly of carbon dioxide. The average temperature on the surface of Mars is –55°C with a pressure of 0.00634 atm. Compare the density of CO2 on Mars’s surface with that on the Earth’s surface at 20°C and one atmosphere. (density on mars/density on earth=blank/1)
Calculate the number of kilojoules of energy required to convert 75.0 grams of solid t-butanol initially at a temperature of -25.0°C to gas at 82.4°C. kJ substance Ethanol Water DMSO t-Butanol formula C₂H5OH H₂O C₂HGSO C4H10O m.w. g/mol m.p. °C 46.069 -114.0 18.015 0.0 78.129 19.0 74.123 25.2 b.p °C 78.0 100.0 189.0 82.4 AH fus AHvap kJ/mol kJ/mol 5.02 38.6 6.01 40.67 14.4 48.6 6.78 39.1 Specific Heat Capacity Liquid J/g.°C 2.30 Solid J/g.°C 0.970 2.09 1.80 1.97 4.184 1.96 2.9 Gas J/g °C 1.94 1.84 1.20 1.73
Consider separate 1.0-L gaseous samples of He, Kr, Cl2, and O2 all at STP. a Rank the gases in order of increasing average kinetic energy. O (KE)avg (He) < (KE),vg (Kr) < (KE)avg (Cl2) = (KE),vg (O2) O (KE)avg (He) = (KE)avg (Kr) < (KE)avg (Cl2) < (KE),vg (O2) O (KE)avg (Kr) < (KE),vg(Cl2) = (KE),vg (O2) < (KE),vg (He) (KE)avg (He) = (KE),vg (Kr) = (KE)vg (Cl2) = (KE),vg (O2) b Rank the gases in order of increasing average velocity. Uavg (Kr) = uavg (Cl2) = uavg (He) = uavg (O2) O uavg (Kr) < uavg (Cl2) < uavg (He) < uavg (O2) O Uavg (Kr) < uavg (O2) < Uavg (Cl2) < Uavg (He) O uavg (Kr) < uavg (Cl2) < Uavg (O2) < uavg (He) C How can separate 1.0-L samples of O2 and He each have the same average velocity? Separate samples of He and O2 can only have the same average velocities if the temperature of the O2 sample is He sample. - the temperature of the
Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO,) into solid calcium oxide and gaseous carbon dioxide. ? 2. Suppose 11.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 360.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.
7. When detern ing the mass of a liquid, ras in a hurry and did not allow enough time for the temperature of the flask to reach the temperature of the boiling water bath. The student recorded the temperature of the gas as 100.0°C when it was only 80.0°C, Is the molar mass calculated by the student higher or lower than the accepted molar mass, or does this error have no effect on the calculated result? Briefly explain your answer # 2/HB Office DEPOTS b) If the student assumed the volume of the flask was 125 mL (as marked by the side of the flask) rather than measuring the volume experimentally, would the unknown's calculated molar mass be too high, too low, or unaffected? Explain. # 2/HB 4
A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into gaseous products. The cylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a large insulated water bath. (See sketch at right.) 1 atm pressure piston cylinder From previous experiments, this chemical reaction is known to absorb 257. kJ of energy. water bath gases The position of the piston is monitored, and it is determined from this data that the piston does 231. kJ of work on the system during the reaction. exothermic Is the reaction exothermic or endothermic? endothermic up Does the temperature of the water bath go up or down? down neither in Does the piston move in or out? out neither in Does heat flow into or out of the gas mixture? out neither How much heat flows? Be sure your answer has the correct number of significant digits.
A two-layer catalytic converter has been designed for diesel engines in automobiles. The first layer in the catalytic converter removes some nitrogen monoxide gas from the exhaust gas and converts it to ammonia gas. In the second layer, ammonia gas is removed as it reacts with the remaining nitrogen monoxide gas. The reactions in the two layers occur at 300°C and are represented by equations I and II. Equation I Equation II 2NO(g) + 3H₂(g) 4NH₂(g) + 6NO(g) catalyst catalyst 2NH₂(g) + O₂(g) +5N₂(g) + 6H₂O(g) ARH° -274.4 kJ ARH° -1815.0kJ The molar enthalpy of reaction for NH3(g) in the reaction represented by Equation II is Record your 5-digit answer. Include sign; do not include units. kJ/mol
BIOL 1603: Org & Evol - Google x A ALEKS - Katie Matthews - Grac x Content app.101edu.co → C esc 1 F1 A glass container was initially charged with 1.50 moles of a gas sample at 5.00 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 33.1 °C, so the final pressure in the container was reduced to 1.50 atm. How many moles of the gas sample are present at the end? Q 2 F2 W # 3 80 E $ 4 F4 R % 675 뽀 F5 T 6 X Question 38 of 66 F6 Y Aktiv Chemistry & 7 F7 U * 00 8 DII F8 ( 1 9 X a Amazon.com: wireles F9 0 1 2 4 7 +/- 0 7 F10 5 8 P
The world burns approximately 3.7 * 1012 kg of fossil fuel per year. Use the combustion of octane as the representative reaction and determine the mass of carbon dioxide (the most significant greenhouse gas) formed per year. The current concentration of carbon dioxide in the atmosphere is approximately 399 ppm (by volume). By what percentage does the concentration increase each year due to fossil fuel combustion? Approximate the average properties of the entire atmosphere by assuming that the atmosphere extends from sea level to 15 km and that it has an average pressure of 381 torr and average temperature of 275 K. Assume Earth is a perfect sphere with a radius of 6371 km.