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 release 193. kJ of energy. water bath The position of the piston is monitored, and it is determined from this data that the piston does 309. kJ of work on the gases system during the reaction. O exothermic Is the reaction exothermic or endothermic? O endothermic O up Does the temperature of the water bath go up or down? O down O neither O in Does the piston move in or out? O out O neither O in Does heat flow into or out of the gas mixture? O out O neither How much heat flows? Be sure your answer has the correct number of significant digits.

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 release 193. kJ of energy. water bath The position of the piston is monitored, and it is determined from this data that the piston does 309. kJ of work on the gases system during the reaction. O exothermic Is the reaction exothermic or endothermic? O endothermic O up Does the temperature of the water bath go up or down? O down O neither O in Does the piston move in or out? O out O neither O in Does heat flow into or out of the gas mixture? O out O neither How much heat flows? Be sure your answer has the correct number of significant digits.

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

A 10.7 g sample of aluminum at 85.3 0C is added to 117 mL of water initially at 14.6 0C. Assuming no heat is lost to the surroundings, calculate the final temperature of the system.
You are baking some cookies for your holiday party this weekend. You add 1/2 teaspoon of baking soda(sodium bicarbonate, NaHCO3) to the cookie dough. When heated, the baking soda releases carbon dioxide (CO2) gas causing the cookies to rise. Balance the chemical reaction below. Calculate the volume of CO2 gas produced in liters when the baking soda is heated in the over at 375 degrees F at 84.0 kPa. Useful information: 1 tsp = 4.6 grams NaHCO3
2. For each of the following sets of data, calculate the missing quantity. Assume that the amount of gas remains constant. SHOW WORK a. V = 8.45 L, at 1.64 atm and 32.0 °C; V = 6.15 L, at ? _atm and 32.0 °C. b. V = 5.82 L, at 1.09 atm and 21.0 °C; V = ? , at 2.75 atm and 45.0 °C.
A prototype sports ball for a new game is precisely inflated to a pressure of 7.3 psi at 25 degrees C. The ball is spherical with an inner bladder diameter of 22.8 cm. It is filled with air (Mw=28.97 g/mol). Not Avogadro’s number is 6.022 x 10^23 atom/mol. A. Calculate the number of moles of air in the ball at the specified temperature and pressure. Consider the air in the ball to follow the ideal gas law. PV=nRT Where P is the absolute pressure of the air in atm, V is the volume of the ball, T is the absolute temperature in K, and R is the ideal gas constant. B. How many oxygen atoms compose the air in the ball? Assume that the mole fraction of N2 in the air is 0.79 and the remainder of the air is 02(oxygen).
What amount of heat is required to convert 10.9 g of an unknown liquid (MM 83.21 g/mol) at 19.2°C to a gas at 93.5 °C? (heat capacity of iquid 1.58 J/g.C; heat capacity of gas 0.932 JIg.°C; AHvap 22.5kJ/mol, Tb= 57.3°C) kJ
Assuming that the natural gas used in a lab is pure methane, CH4, write a balanced chemical equation for the reaction of natural gas with each of the copper oxides, (Red copper oxide Cu2O, and Black copper oxide, CuO). Assume the products for both reactions are copper metal, water vapor, and carbon dioxide gas. Include all phases in the reactions.
1a. Calculate the pressure of a sample of 1 mole of argon gas in a 0.1500 L flask at -10.2 ℃ using the ideal gas law and the Van der Waals equation. The a value for argon is 1.34 (L 2 ∙ atm/mol2 ) and the b value is 0.0322 (L/mol). Show all work Ideal pressure= ? real pressure =? 1b.Why is there a difference in the real gas pressure and the ideal pressure? Explain what assumption(s) of the kinetic molecular theory of gases break down under these conditions.
Q:15 A sealed metal canister at 749 torr pressure is heated from -25.0 °C to 100 °C. What is the final pressure in atm? (show work)
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
1. A 1.0L flask contains equal amounts of O2 and CO2 at 25°C. a. Which molecules have the greater average speed or are they the same? b. Which molecules have the greater average kinetic energy or are they the same?
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 (CaCO2) into solid calcium oxide and gaseous carbon dioxide. C 2. Suppose 86.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 260.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.