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.) From previous experiments, this chemical reaction is known to absorb 278. kJ of energy. The temperature of the water bath is monitored, and it is determined from this data that 285. kJ of heat flows into the 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? Round your answer to 1 significant digit.

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.) From previous experiments, this chemical reaction is known to absorb 278. kJ of energy. The temperature of the water bath is monitored, and it is determined from this data that 285. kJ of heat flows into the 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? Round your answer to 1 significant digit.

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

Related questions

Q: thermometer A sample of quartz, which has a specific heat capacity of 0.730 J-g is put into a…

Q: A 10.0 kg sample of water is used to cool a hot engine. How much heat is removed from the engine if…

A: Molar heat capacity (Cp) :- The amount of heat required to rise the temperature of one mole of a…

Q: A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into…

Q: A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas…

A: We know the expression of the ideal gas equation : => PV = nRT where, V is the volume, n is the…

Q: A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into…

A: To answer: Is the reaction exothermic or endothermic? Does the temperature of the water bath go up…

Q: thermometer A 58.8 g sample of quartz, which has a specific heat capacity of 0.730 J•g '.°C', is put…

Q: 250 mL of water initially at 15 °C is heated by adding 6.7 kJ of heat using a gas burner. Calculate…

A: Since the heat added to the water and temperature change is related by Q = mCΔT where Q = heat…

Q: thermometer- A 52.2 g sample of brass, which has a specific heat capacity of 0.375 J-g1C1, is put…

A: Given mass of brass (mb) = 52.2 g mass of water (mw) = 200 gspecific heat of brass (cb) = 0.375…

Q: A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains…

Q: Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according…

A: enthalpy of reaction is energy needed for completion of the reaction.

Q: A student obtained a clean flask. She weighed the flask and stopper on an analytical balance and…

Q: A foundry worker places a 5.77 kg sheet of cobalt at a temperature of 15°C on top of a 16.8 kg sheet…

Q: A 30.1-g sample of water at 300. K is mixed with 51.3 g water at 340. K. Calculate the final…

A: In the above it is given that , no heat is loss to the surrounding . Means heat lost by hot water…

Q: A block of Iron metal is heated to 180.0oC and then dropped into 50.0 g of water initially at…

A: The heat required to raise the temperature of a sample of mass 'm' having specific heat 'c' from T1…

Q: A sample of brass, which has a specific heat contains 200.0 g of water. The brass sample the…

A: Loss of Heat of the Metal brass = Gain of Heat by the Water -Qbrass = Q water Q = mC∆T -mC ∆T for…

Q: moles of an ideal gas in a volume of 6.00 L with a pressure of 1.00 atm. The cylinder is surrounded…

Q: We have a calorimetric bomb with a heat capacity of 555 J/K. The bomb is filled with 1000.0 mL of…

A: Anser:A bomb calorimeter is a common equipment used to determine the heat associated with a certain…

Q: A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas…

A: Answer:Here:

Q: 31.4-g sample of water at 290. K is mixed with 50.7 g water at 340. K. Calculate the final…

A: If you assume that no heat is lost to the surroundings, then you can say that the heat lost by the…

Q: thermometer -1 A 53.2 g sample of quartz, which has a specific heat capacity of 0.730 J'g *°c ', is…

A: Given data, mass of quartz = m=53.2 g, Cp for quartz=0.730 J g-1 ℃ Equilibrium temperature T2=23.4℃…

Q: is put into a calorimeter (see sketch at right) that A sample of glass, which has a specific heat…

Q: A 25.4-g sample of water at 290. K is mixed with 47.3 g water at 350. K. Calculate the final…

A: Let final temperature be T, the heat gained or heat absorbed by 25.4 g of water (q1) is determined…

Q: The heater used in a 4.32 m×3.69 m×3.01 m4.32 m×3.69 m×3.01 m dorm room uses the combustion of…

A: Given that : The dimension of the room = 4.32 m×3.69 m×3.01 m The specific heat of air is 30.0…

Q: thermometer. A sample of brass, which has a specific heat capacity of 0.375 J-g.°C , is put into a…

Q: thermometer A sample of glass, which has a specific heat capacity of 0.670 J•g¯.°C¯', is put into a…

A: Given mass of water = 200 g Initial temperature of water = 15°C Final temperature of water = 18.6°C…

Q: 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…

A: Given, Mass of aluminum = 10.7g. Initial temperature of aluminum = 85.3oC. Mass of water = 117mL =…

Q: thermometer. A sample of aluminum, which has a specific heat capacity of 0.897 J'g.°C', is put into…

Q: thermometer- A 57.9 g sample of quartz, which has a specific heat capacity of 0.730 J-g¹c¹, is put…

Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

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
pist
From previous experiments, this chemical reaction is known to absorb 278. kJ of energy.
The temperature of the water bath is monitored, and it is determined from this data that 285. kJ of heat flows into the
system during the reaction.
gases
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
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? Round your answer to 1 significant
digit.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A coin dealer, offered a rare silver coin, suspected that it might be a counterfeit nickel copy. The dealer heated the coin, which weighed 16.0 g to 100°C in boiling water and then dropped the hot coin into 29.0 g of water at T = 18.0°C in an insulated coffee-cup, and measured the rise in temperature. If the coin was really made of silver, what would the final temperature of the water be (in °C)? (for nickel, s = 0.445 J/g°C; for silver, s = 0.233 J/g°C )
Every day a certain amount of water evaporates from Earth’s oceans, lakes, and land surface and forms water vapor and clouds in the atmosphere. Every day a certain amount of rain falls back to Earth. Make the reasonable assumption that, on average, the energy absorbed by the evaporation and lifting of the water is equal to the energy released by its condensation and falling back to earth. The evaporation of one mole of water requires approximately 40.6×103 J of heat. An equal amount of heat is released when a mole of water condenses. The annual volume of rainfall on Earth is approximately 4.9×105 km3 and the average cloud altitude is 8.9 km above Earth’s surface. How much energy, in joules, is required every day to evaporate and lift the water?
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)
A sample of iron, which has a specific heat capacity of 0.449 J.g¹.°C¹, is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The iron sample starts off at 98.2 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 27.4 °C. The pressure remains constant at 1 atm. Calculate the mass of the iron sample. Be sure your answer is rounded to 2 significant digits. 1 g x10 X 5 thermometer. insulated container water sample a calorimeter
A 102.8 g sample of a metal initially at 183.00C is placed in 35.0 ml of water initially at 25.0 0C. After reaching thermal equilibrium, the final temperature of the system is 58.80C. What is the identity of the metal? Assume no heat is lost to the surroundings.
I A sample of aluminum, which has a specific heat capacity of 0.897 J.g .°C is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The aluminum sample starts off at 85.5 °C and the temperature of the water starts off at 16.0 °C. When the temperature of the water stops changing it's 23.3 °C. The pressure remains constant at 1 atm. Calculate the mass of the aluminum sample. Be sure your answer is rounded to the correct number of significant digits. thermometer. insulated container water sample a calorimeter