5.2 b Calculate the magnitude of q for a system that does 7.05 × 105 kJ of work on its surroundings and for which the change in total internal energy is −9.55 × 103 kJ. Indicate whether heat is absorbed or released by the system.

Q: The specific heat capacity of lead at 25°C is 1.290×10-1 J/g/K. Answer the following: (a) For a…

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Q: (a) Consider the following chemical reaction: 3FE203(s) + C0(g) → 2FE304(s) + CO2(g) AH° = ? Use the…

A: Thermodynamics is the branch of chemistry that mainly deals with the heat transfer between system…

Q: . (a) We place 77.7 g of a metal at 10.00 ◦C in 333.3 g of water at 70.00 ◦C. The water is in a…

A: Dear student, we are authorised to solve only one question at a time. Please post rest of the…

Q: A system takes in 0.430 kJ of heat while it does 0.830 kJ of work on the surroundings. What is the…

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Q: What is the change in internal energy for a system which loses 422 J of heat, and on which 227 J of…

A: According to first law of thermodynamics the change in internal energy is expressed as shown below:

Q: A sample of benzene, C6H6, weighing 3.51 g was burned in an excess of oxygen in a bomb calorimeter.…

A: q= m c ∆Tq=Heat absorbed or evolvedm=mass of substancec=specific heat capacity∆T=final…

Q: Calculate q, and determine whether heat is absorbed or released when a system does work on the…

A: Sign convention: Work done by the system on the surrounding = negative (-) Work done on the system…

Q: A system gains 612 kJ of heat, resulting in a change in internal energy of the system equal to +181…

A: Given,Heat gain (Q)=612kJChange in internal energy(∆U)=181kJ

Q: A generic solid, X, has a molar mass of 59.5 g/mol. In a constant‑pressure calorimeter, 45.3 g of X…

A: The heat absorbed by the solution on dissolution of a generic solid can be calculated by the…

Q: What is the change in the internal energy of the system if the surroundings releases 300J of heat…

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Q: The internal energy of a gas decreases by 1.65kj when it transfers 1.87kj of energy in the form of…

A: Interpretation: The work done on the gas by the surroundings is to be determined. Concept…

Q: A 1.110-g sample of benzoic acid (HC7H5O2; molar mass = 122.12 g/mol) is burned in an excess of…

A: This problem can be solved by using the equation :                             q=mc∆Twhere q is the…

Q: A system absorbs 1.66E2 kJ of heat and the surroundings do 1.032E2 kJ of work on the system. What is…

A: We have to predict the change in internal energy of system.

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: chemical reaction requires 369.42 kJ of heat and performs 73.7 kJ of work on the surroundings. What…

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Q: suppose that a system gives off 50.1 kJ of heat and has 300. J of work done on it.   What is the…

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Q: A sample of benzene, C6 H6, weighing 3.51 g was burned in an excess of oxygen in a bomb calorimeter.…

A:

Q: A system does 546 kJ of work and loses 271 kJ of heat to the surroundings. What is the change in…

A: Work (w) = -546 KJ (because work is done on the surrounding, so this is negative) Heat (q) = -271 KJ…

Q: One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 6.00 liters against…

A: Given: Initial volume = 1.00 liter Final volume  = 6.00 liter Pressure         = 1 atm Heat released…

Q: Calculate ΔE , if the system absorbs 7.24 kJ of heat from the surroundings while its volume remains…

A: Since the volume is remaining constant and we know that work done = -PΔV => Work = 0 as volume is…

Q: 13.00 g of Compound X with molecular formula C4H, are burned in a constant-pressure calorimeter…

A: Answer:Enthalpy change during the formation of 1 mole of a compound from its elements in their…

Q: (b) A student heats up some soup in a pot on a stove. If the student did o.25 kJ of work on the soup…

A: Work done (W) by the system is ‘-’ and work done (W) on the system is‘+’. Heat absorbed (q) by the…

Q: An experiment is performed in the chemical lab, 405 J of heat is absorbed by a system and 285 J of…

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Q: Calculate ΔE of a gas for a process in which the gas evolves 24 J of heat and has 9 J of work done…

A: Applying 1st law of thermodynamics  ΔE = q + w  where ΔE is change in internal energy , q = heat…

Q: Given: 4AICI3(s) + 302(g) → 2Al,O3(s) + 6C12(g); AH=-529.0 kJ determine AH for the following…

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Q: An ideal gas sealed in a rigid 4.50-L cylinder, initially at pressure Pi=12.30 atm, is cooled until…

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Q: An ideal gas sealed in a rigid 3.13-L cylinder, initially at pressure Pi=12.70 atm, is cooled until…

A: Given information, Volume of gas = 3.13 L Initial pressure (Pi) = 12.70 atm Final pressure (Pf) =…

Q: A system gains 667 kJ667 kJ of heat, resulting in a change in internal energy of the system equal to…

A: According to the first law of thermodynamics; Consider the given information is as follows;…

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: Calculate the internal energy change (ΔE) for a system undergoing an exothermic process in which…

A: Given , Since the process is exothermic. So q will be negative. Heat , q = - 24.9 kJ Work done on…