Answered: Calculate (a) q when a system does 55 J…

Calculate (a) q when a system does 55 J of work and its energy decreases by 68 J and (b) AE for a gas that releases 31 J of heat and has 115 J of work done on it. a. q |J b. ΔΕ J

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.18PAE: 9.18 Calculate (a) q when a system does 54J of work and its energy decreases by 72 J and (b) E for a...

See similar textbooks

Related questions

Q: A gas expands and does P-V work on the surroundings equal to 294 J. At the same time, it absorbs 246…

A: The first law of thermodynamics states that the change in internal energy of a system equals the net…

Q: The AU of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is J. O…

A: Detail mathematical calculation is shown below to find out the change in internal energy

Q: What is the specific heat capacity of a metal if it requires 269.6 J to change the temperature of…

A: q=ms∆T Putting these values.

Q: 5.2 b Calculate the magnitude of q for a system that does 7.05 × 105 kJ of work on its surroundings…

A: From given data W = -7.05×105 kJ ∆U = -9.55×103 kJ W is negative because work is done by system on…

Q: The standard enthalpies of combustion at 25°C of hydrogen gas, H2(g), n-butane – C4H10(g), 1-butene…

Q: If a system has 5.00 x 10° kcal of work done to it, and releases 5.00 x 10' kJ of heat into its…

A: Since you have posted multiple questions, we are entitled to answer the first only. 1) Given: Work…

Q: A 50.0 g sample of scandium, Sc, is heated by exposure to 1.50 x 10J. The temperature of the Sc is…

A: Given: Mass of water = 50.0 g Heat energy = 1.50×10 J Change in temperature = 61.1 oC

Q: A system does 566 kJ of work and loses 216 kJ of heat to the surroundings. What is the change in…

Q: The standard enthalpy change for the following reaction is 1.11x10 kJ at 298 K. 2 BaO(s) 2 Ba(s) +…

A: By Hess's law of constant heat summation: Equation (ii) = -1/2 x equation (i) ∆H2° = -12×∆H1° ∆H2°…

Q: 1. A sample of metal with mass 250.0 g is heated to 130.0 ℃ and dropped into 425 g of water at 26.0…

Q: When a system gives off heat and does not work on its surroundings, delta E is always(

A: According to the First law of thermodynamics, ∆E = q + W Here, q = Heat released or absorbed.…

Q: An electric battery is charged by supplying 250 kJ of energy to it as electrical work, but in the…

A: Answer:- This question is answered by using the simple concept of calculation of change in the…

Q: If a system has 325 keal of work done to it, and releases S5.00 x 10 kJ of heat into its…

Q: When 15.3 g of sodium nitrate was dissolved in water in a calorimeter, the temperature fell from…

Q: If a system has 375 kcal of work done to it, and releases 5.00 x 10 kJ of heat into its…

A: Given is Work done on system w = 375 kcal = 1569 kJ [since 1cal = 4.184 J ] Heat released by…

Q: A gas is compressed in a piston with 8.80E1 J of work. As a result, 4.2E1 J of heat is given off to…

A: Solving only first question in accordance with the guidelines. We will answer this question using…

Q: 4-A system suffers an increase in internal energy of 80 J and at the same time has 50 J of work done…

Q: During an experiment, a student adds 1.23 g Ca0 to 200.0 mL of 0.500 M HCI. The student observes a…

A: Generally the heat released in the reaction is absorbed by the solution and raises the temperature…

Q: If 800 J of heat is added to a system when it does 500 J of work, what is the change in internal…

Q: Calculate (a) q when a system does 49 J of work and its energy decreases by 70. J and (b) AE for a…

A: (a) The given data is as follows: The work done by the system = -49 J (negative sign is there as…

Q: A gas expands and does P-V work in the surroundings equal to 279 J. At the same time, it absorbs…

Q: 1. What and expound the First law of Thermodynamics? 2. Define in your own words A. Specific heat B.…

A: What is first law of thermodynamic, explanation is given below.

Q: 1. Find the change in the internal energy when 175 J of work is done on a system that evolves 50 J…

A: Given:Heat (q) = 50 J Work (W) = 175 J since, work is done on the system which means energy…

Q: How much work, w, must be done on a system to decrease its volume from 12.0 L to 3.0 L by exerting a…

A: w = P . ∆V P = 3.0 atm and ∆V = 12.0 - 3.0 = 9.0 L w = 3.0 x 9.0 = 27.00 L. atm

Q: What is the AE of a system if 184 kJ of work is done on the system and it loses 267 kJ of heat?

A: We use the first law of thermodynamic for calculating the change in internal energy. This low state…

Q: A calorimeter contains 16.0 mL of water at 14.5 °C. When 2.20 g of X (a substance with molar mass of…

A: Given : Mass of X = 2.20 g Volume of water = 16.0 mL Heat capacity (C) = 4.18 ∆T = 25.5 - 14.5 =…

Q: (SHOW CALCULATIONS) A system delivers 1525 J of heat while the surroundings perform 860 of work on…

A: Given : Heat delivers by system = 1525 J Work performed by surrounding on system = 860 J

Q: 3. When 1.38 g of liquid PCl; at 25.55 "C is added to 1.00 x 10g of water at 25.55 "C in a…

A: Given: Mass of PCl3 dissolved = 1.38 g. Initial temperature = 25.55 oC Mass of water = 100 g. And…

Q: A system gains 727 kJ727 kJ of heat, resulting in a change in internal energy of the system equal to…

A: As we know; deltaU = Q + W where delta U is change in internal energy Q = heat produced W =…

Q: A typical room in a house contains 5.10 x 104 L of air (density = 1.29 g/L). How many moles of…

A: Specific heat capacity is the amount of heat that is required to rise a temperature of 1 kg…

Q: If a system has 375 kcal of work done to it, and releases 5.00 x 10² kJ of heat into its…

Q: When 0.0200 L of 0.800 M NaOH is mixed with 0.0400 L of 0.400 M HNO3 in a coffee-cup calorimeter,…

A: The amount of heat released in the process of neutralization is absorbed by the coffee-cup…

Q: 5.4 The contents of the closed box in each of the following illustra- tions represent a system, and…

A: The first law of thermodynamics describes that energy can neither created nor destroyed, it can be…

Q: What is the internal energy of the system that absorbs 90 J of heat and 15 J work done by the…

Q: 17D.1. (a) What is the specific heat of liquid water? (b) What is the molar heat capacity of liquid…

A: Specific heat is the amount of heat per unit mass required to raise the temperature by one degree…

Q: According to the First Law of Thermodynamics, a system which absorbs 40 J of heat and produces 20 J…

Q: The enthalpy for the formation of 1 mole of NH3(aq)NH3(aq) is -80.29 kJ/molkJ/mol. What is the…

A: The standard molar enthalpy of formation is defined as the standard change in enthalpy for the…

Q: You discover a new substance and wish to determine its specific heat capacity. Your sample weighs…

Q: temperature of the calorimeter increases from 22.14°C to 26.82°C. What is the heat of combustion per…

A: #(a): Given: Initial temperature of the calorimeter, Ti = 22.25 oC Final temperature of the…

Q: Calculate (a) q when a system does 43 J of work and its energy decreases by 70. J and (b) AE for a…

A: A) given: Work done = 43 J Energy decreases by = 70 J B) Heat released = 36 J Work done = 107 J

Q: When 50.0 mL of 1.27 M of HCl(aq) is combined with 50.0 mL of 1.32 M of NaOH(aq) in a coffee-cup…

Q: a system does 596 kJ of work and loses 276 kJ of heat to the surroundings. What is the change in…

A: According to first law of thermodynamic, The total internal energy is

Q: If a system has 475 kcal of work done to it, and releases 5.00 x 102 kJ of heat into its…

Q: Ethanol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. The standard…

Q: If a system has 225 kcal of work done to it, and releases 5.00 x 10² kJ of heat into its…

A: Given, Work done on the system W=225 Kcal {As work is done by the system , so W is +ve} Heat…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.34 kg sample…

A: Mol= weight/ molar mass first find the moles in 0.34kg

Q: The value of ΔE for a system that performs 190 kJ of work on its surroundings and gains 250 kJ of…

Q: 2- Calculate the total internal energy change (AU) for a system that loses 50 J of heat and gains…

A: According to the 1st law of thermodynamics :- △U=q+Wwhere , △U=Change in internal…

Q: -. The contents of the closed box in each of the following illustrations represent a system, and the…

A: Since numerical values of w or Q are not given, we have to use sign convention to find the sign of…

Q: What is the heat energy required to raise the temperature of 5 grams of lead from 10 ̊C to 15 ̊C?

A: q = mc∆T q is the amount of heat energy required m is the mass of lead c is the specific heat…

Question

Calculate (a) q when a system does 55 J of work and its energy decreases by 68 J and
(b) AE for a gas that releases 31 J of heat and has 115 J of work done on it.
a. q
|J
b. ΔΕ
J

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

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 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?
9.53 Using these reactions, find the standard enthalpy change for the formation of 1 mol of PhO(s) from lead metal and oxygen gas. PbO(s)+C(graphite)Pb(s)+CO(g) H = 106.8 kJ 2C(graphite)+O2(g)2CO(g) H= -221.0 kJ If 250 g of lead reacts with oxygen to form lead(II) oxide, what quantity of thermal energy (in kJ) is ahsorhed or evolved?
A piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil, the current, and the Time the current flowed, it was calculated that 235 J of heat was added to the lead. The temperature of the lead rose from 20.4C to 35.5C. What is the specific heat of the lead?
The complete combustion of acetylene, C2H2(g), produces 1300. kJ of energy per mole of acetylene consumed. How many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal water by 10.0c if the process is 80.0% efficient? Assume the density of water is 1.00 g/cm3
Nitrogen gas (2.75 L) is confined in a cylinder under constant atmospheric pressure (1.01 105 pascals). The volume of gas decreases to 2.10 L when 485 J of energy is transferred as heat to the surroundings. What is the change in internal energy of the gas?
Principles of Heat Flow Titanium is a metal used in jet engines. Its specific heat is 0.523 J/g C. If S.SS g of titanium absorb 4.78 J, what is the change in temperature?
A piece of unknown solid substance weighs 437.2 g, and requires 8460 J to increase its temperature from 19.3 °C to 68.9 °C. (a) What is the specific heat of the substance? (b) If it is one of the substances found in Table 5.1, what is its likely identity?
9.18 Calculate (a) q when a system does 54J of work and its energy decreases by 72 J and (b) E for a gas that releases 38 J of heat and has 102 J of work done on it.
You did an experiment in which you found that 59.8 J was required to raise the temperature of 25.0 g of ethylene glycol (a compound used as antifreeze in automobile engines) by 1.00 K. Calculate the specific heat capacity of ethylene glycol from these data.
How much heat is produced when loo mL of 0.250 M HCl (density, 1.00 g/mL) and 200 mL of 0.150 M NaOH (density, 1.00 g/mL) are mixed? HCl(aq)+NaO(aq)NaCl(aq)+H2O(l)H298=58kJ If both solutions are at the same temperature and the heat capacity of the products is 4.19 J/g C, how much will the temperature increase? What assumption did you make in your calculation?
Combustion of table sugar produces CO2(g) and H2O( l). When 1.46 g table sugar is combusted in a constant-volume (bomb) calorimeter, 24.00 kJ of heat is liberated. a. Assuming that table sugar is pure sucrose, C12H22O11 (s), write the balanced equation for the combustion reaction. b. Calculate E in kJ/mol C12H22O11 for the combustion reaction of sucrose.