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 160. kJ of energy. water bath The temperature of the water bath is monitored, and it is determined from this data that 248. kJ of heat flows out of 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 does work Does the gas mixture do work, or is work done on it? O work is done on it O neither How much work is done on (or by) the gas mixture? Be sure your answer has the correct | kJ

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 160. kJ of energy. water bath The temperature of the water bath is monitored, and it is determined from this data that 248. kJ of heat flows out of 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 does work Does the gas mixture do work, or is work done on it? O work is done on it O neither How much work is done on (or by) the gas mixture? Be sure your answer has the correct | kJ

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

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 (CaCO3) into solid calcium oxide and gaseous carbon dioxide. 2. Suppose 85.0L of carbon dioxide gas are produced by this reaction, at a temperature of 210.0°C and pressure of exactly 1atm. Calculate the mass of calcium carbonate that must have reacted. Be sure your answer has the correct number of significant digits.
thermometer A sample of quartz, which has a specific heat capacity of 0.730 J'g c, is put into a calorimeter (see sketch at right) that contains 150.0 g of water. The quartz sample starts off at 85.2 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 159.1 °C. The pressure remains constant at 1 atm. insulated container water Calculate the mass of the quartz sample. Be sure your answer is rounded to the correct number of significant digits. sample a calorimeter
Nadine needs to heat 2.0 L of water from 15ᵒC to 90ᵒC. A) how much energy is needed to heat the water? B) If burning methane (CH4) releases 810 kJ/ mole, what mass of methane will be burned? C) What volume of oxygen at 20ᵒC and 725 mmHg will be consumed by the combustion of methane? You will need a balanced equation and a gas law for C and the specific heat capacity of water is 4.184J/gᵒC.
21 Consider the combustion of in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. C₅H₈ (l) + 7 O₂ (g) → 5 CO₂ (g) + 4 H₂O (g) d If 4790 J of heat were absorbed by the water, then how much heat, in J, was produced by the combustion of C₅H₈? (include the appropriate sign)
thermometer- A 56.5 g sample of iron is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The iron sample starts off at insulated container 89.3 °C and the temperature of the water starts off at 17.0 °C. When the temperature of the water stops changing it's 19.2 °C. The pressure remains constant at l atm. water Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to the correct number of significant digits. sample a calorimeter
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.
A sample of gass occupies a volume of 56.4mL. As it expands, it does 133.3J of work on its surroundings at a constant pressure of 783 torr. What is the final volume of gas?
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 (CaCO3) into solid calcium oxide and gaseous carbon dioxide. x10 2. ose 20.0 L of carbon dioxide gas produced by this reaction, at a temperature of 370.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.
An electric heater supplies 43.3 joules of energy to 27.3-g sample of H2 gas originally at 27.6 °C. Compute the final temperature (in °C). i °C
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.
A sample of glass, which has a specific heat capacity of 0.670 J-gec, is put into a calorimeter (see sketch at right) that insulated container contains 250.0 g of water. The glass sample starts off at 86.1 °C and the temperature of the water starts off at 18.0 °C. When the temperature of the water stops changing it's 20.3 "C. The pressure remains constant at 1 atm. Calculate the mass of the glass sample. Be sure your answer is rounded to the correct number of significant digits. 18 D.P thermometer- X water sample a calorimeter Ar
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.