The PV dilute gas diagram is shown in the figure opposite. In this process, assuming that the internal energy is 456J at one point and 223J at two points. How much heat has been exchanged? Has the gas gained or lost heat?

Q: An automobile engine provides 581 Joules of work to push the pistons and generates 2167 Joules of…

A: The relationship between change in internal energy (∆E), heat (q) and work done (W) is given by…

Q: A 56.59 g sample of a substance is initially at 25.6 °C. After absorbing 2789 J of heat, the…

A:

Q: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g…

A: Heat change in a body is depends on the mass and temperature change of the body. heat change = mass…

Q: A chemist must add 3,352 kJ of heat to 2 mol solid Al2O3 to cause it to break down to form 4 mol…

A: Given: Heat supplied to solid Al2O3 = 3352kJno of moles of Al2O3 taken  = 2molno of mol of Al formed…

Q: If 46.1g of copper at 11.6 degrees is place in 85.0g of water at 72.4 degrees what is the final…

A: Heat loss is given by the formula           -q = mC∆T     Or      -q = mC(Tf - Ti)  Where,  q=…

Q: Consider a cold can of soft drink on a table in a warm room.  If the cold can of soft drink is the…

A: According to the first law of thermodynamics, the energy of the universe remains constant. For a…

Q: A 1.69 gram sample is heated to an initial temperature of 75 oC. The sample is then placed in a…

A:

Q: An automobile engine provides 519 Joules of work to push the pistons. In this process the internal…

A: According to first law of thermodynamics , the relationship between change in internal energy , heat…

Q: A gas is compressed from an initial volume of 5.55 L to a finalvolume of 1.22 L by an external…

A: The expression for the work done,  W=-P(Vf-Vi)W=-1.00 atm (1.22 L-5.55 L)W=4.33 L (101.33 J)1 L…

Q: Perform the following heat calculation.  show all work and include units on answer A 45.4 g sample…

A:

Q: 479.1 g sample of silicon dioxide undergoes a temperature change of -87.43 K while releasing 29447…

A: Heat absorbed/released, q = mCs∆T  m = mass of substance Cs = specific heat capacity of substance ∆T…

Q: A 150 g sample of a metal is heated to 75.0°C and then placed in a calorimeter containing 150.0 g of…

A: Interpretation -  To determine the specific heat capacity of metal when a 150g of metal is heated to…

Q: A 25.00 g piece of metal was heated at 100 degrees Celsius and was introduced to into a calorimeter,…

A: The given problem can be solved by using the formula given below as; -Qmetal=+Qwater…

Q: A student mixes 41.8 g of ethanol at 15.8°C with 50.7 g of water at 49.2°C. If the resulting…

A: To find the answer, just compare the heat that ethanol gains to the heat that water loses. Water…

Q: An automobile engine provides 621 Joules of work to push the pistons. In this process the internal…

A: According to the first law of thermodynamics, the following expression is obtained: ∆U=q+w…

Q: When 1 mol of CS2 (I) forms from its elements at 1 atm and 25.0°C, 89.7 kJ of heat is absorbed. It…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: A 531.6 g sample of sodium undergoes a temperature change of +86.75 °C while absorbing 857.4 joules…

A:

Q: air in an inflated balloon (system) is warmed and absorbes 665. J of heat the surroundings also…

A:

Q: A 27.24 g27.24 g sample of a substance is initially at 26.6 ∘C26.6 ∘C . After absorbing 496 cal496…

A:

Q: A chemist measures the energy change AH during the following reaction: CH₂(g)+202(g) → CO₂(g)+…

A: H of reaction = -882. kJ/molmass of CH4 = 71.1 gmolar mass of CH4 = 16.04 g/mol

Q: A 818 g sample of metal with a specific heat capacity of 0.251 of J/g•ºC is initially at a…

A: Given  Mass = 818 g Heat = 1.5 kJ = 1500 J T1 = 22.6°C Specific heat = 0.251 J/g-°C

Q: A 1.211 g of benzoic acid (CH§ COOH) was ignited in pure oxygen gas and the heat released from the…

A: Here's a step-by-step explanation:1. **Understanding the System**: We have benzoic acid (C6H5COOH)…

Q: When one mole of C6H6C6H6 is burned, 3.27 MJ3.27 MJ of heat is produced. When the heat from burning…

A: The number of moles of C6H6 is 1 mol. The heat released is 3.27 MJ. The weight of C6H6 is 7.87 g.…

Q: A system conducts 255 cal of heat to the surroundings whiledelivering 428 cal of work. What is the…

A: Internal energy is the energy present within the system which rises up when molecular motion takes…

Q: substance is initially at 20.3 ∘C.20.3 ∘C. After absorbing 2063 J2063 J of heat, the temperature of…

A: Heat of reaction is difference of energy of product  and energy of Reactant. If heat of reaction is…

Q: A 2.62E1 g sample of aluminum at 1.008E2 °C is added to 1.002E2 g of water at 2.22E1 °C in a…

A: For a chemical reaction or physical process to occur a certain amount of energy should be furnished…

Q: Which of the following makes sense: When volume of a system is under constant pressure, which of…

A: The enthalpy change is defined as the internal energy change plus product of constant pressure and…

Q: 100 g of water at 86 °C is mixed with 200 g of water at 17 °C. What is the final temperature of the…

A: apply the concept ,  heat taken = heat given

Q: In the laboratory a student finds that it takes 34.3 Joules to increase the temperature of 13.7…

A:

Q: Calculate the energy required to heat 133.0 mg of silver from -6.9 °C to 17.7 °C. Assume the…

A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…

Q: 9. What mass of natural gas (CH4) must burn to emit 3,447 kJ of heat? CH4 (g) + 202 (g) → CO2 (g) +…

A: The mass of CH4 can be calculated as follows

Q: A chemist measures the energy change AH during the following reaction: 2 NH3(g) → N₂(g) + 3H₂(g) Use…

A:

Q: An electrical heater is used to supply 150.0 J of energy to a 30.0 g sample of aluminum…

A: The specific heat capacity for a given chemical substance or a solution refers to the amount of the…

Q: The system changes from state 1 to state 2 and its internal energy change is -188 J. During the…

A: We have to predict the heat released or heat absorbed.

Q: A chemical reaction (or other process) warms up its container as it happens. The heat for such a…

A: The heat of a system is negative, if heat is released in the system and positive, if heat is gained…

Q: A sample of Ni(s) is heated to 98.8 Celsius and placed into a coffee cup calorimeter containing…

A: Given, mass of water = 150.0 g

Q: A 402 g sample of silicon is subjected to a temperature change of -800.29 K while releasing 228980…

A: Heat released by the material = mass × specific heat capacity ×temperature change Where, heat…

Q: Calculate the energy required to heat 430.0 mg of iron from -2.1 °C to 12.1 °C. Assume the specific…

A:

Q: A solid state substance absorbs 5589kJ of energy. The mass of the substance is 0.774kg. Assuming the…

A:

Q: O Macmillan Learning Introductory Chemistry Revell SECOND EDITION presented by Macmillan Learning A…

A:

Q: Chemistry 1. A pool of lava exhibits Group of answer choices nuclear energy thermal energy…

A: Lava is extremely hot and average temperature is about 750°C .A pool can be used to produced…

Q: An 33.83 g sample of aluminum is placed on a 66.98 g sample of copper initially at 112.55oC. If the…

A: Given: Mass of Aluminum taken = 33.83 g Mass of copper taken = 66.98 g Initial temperature of copper…

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.