The ΔE of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is ________ J.

Q: A 25.0 g block of copper (specific heat capacity 0.380 J/g-°C) at 88.0 °C is placed into 500.0 g of…

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Q: A system does 551 kJ of work and loses 236 kJ of heat to the surroundings. What is the change in…

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Q: When a 4.25-g sample of solid sodium nitrate dissolves in 50.0 g of water in a coffee-cup…

A: The mass of sodium nitrate is = 4.25 g The mass of water is = 50.0 g The mass of solution is =…

Q: The heat of combustion of fructose, C6H12O6, is -2812 KJ/mol. If a fresh golden delicious apple…

A: Molar mass of fructose = 180.16 g/mol

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: Consider the following reactions: 3C(s) +4H,(g)→C;H,(g) AH° =-103.8kJ C(s) +0,(g)→ CO,(g) AH'…

A: Hess’s law- Change in enthalpy for a reaction is independent on path or steps followed by reaction.…

Q: A 25.0 g block of copper (specific heat capacity 0.380 J/g °C) at 32.6 °C is placed into 500.0 g of…

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Q: How much heat (in kJ) is needed to raise the temperature of 100.0 grams of water by 25.0 °C?  The…

A: Mass of water(m) = 100 gm  specific heat capacity of water(s) = 4.184 J/g·°C  Increase in…

Q: 5.114 A 3.52-g sample of ammonium nitrate (NH4NO3)was added to 80.0 mL of water in a…

A: Given that : Mass of ammonium nitrate = 3.52g Mass of water = 80.0mL = 80.0g Change in temperature…

Q: An ideal gas with a volume of 0.1m' expands at a constant pressure of 1.5 x 10ʻPa to tripe its…

A: Given : Constant Pressure = 1.5 X 105 Pa Initial volume = 0.1 m3  And final volume = triple of…

Q: A reaction releases 173 J of energy while doing 42 J of work. Determine the change in internal…

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Q: A sample of sucrose, C12H22O11 weighing 0.1328 g, was burned to completion in a bomb calorimeter at…

A: Given: sucrose sample weight   =   0.1328 g,  Temperature                      = 25°C,…

Q: What is the work involved in a process where a system experiences a net loss of energy equal to 4.6…

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Q: A piece of unknown solid substance weighs 439 g, and requires 8427 J to increase its temperature…

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Q: A chemical system produces 155 kJ of heat and does 22 kJ of work. What is ΔE for the surroundings?a)…

A: In order to solve this question, we will use the first law of thermodynamics which states that…

Q: calculate the amount of heat (in J) necessary to raise the temperature of 23.9 g benzene by 27.0 °C.…

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Q: mass

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Q: 2. An aluminum container with specific heat capacity of 0.880 J/g"C contains waxwith specific heat…

A: Please find the attached images for the answer I am giving the answer for question number 2 only.

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 the same amount of energy in the form of heat is added to 19.5 g samples of each of the metals…

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Q: Consider the thermochemical equation for the combustion of ethyl alcohol: C2H5OH(l)  + 3O2(g)  --->…

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Q: A 25.0 g block of copper (specific heat capacity 0.380 J/g･°C) at 59.8 °C is placed into 500.0 g of…

A: Given data is as follows: The mass of copper = 25.0 g The specific heat capacity of copper = 0.380…

Q: Determine the efficiency of a camp stove given the following data: mass of propane burned = 4.48 g…

A: Interpretation- We have to determine the effciency of a camp stove on the basis of data as given…

Q: A 25.0 g block of copper (specific heat capacity 0.380 J/g･°C) at 44.6 °C is placed into 500.0 g of…

A: We have to calculate the change in temperature for metal block.

Q: 4. A 50.0 gram piece of hot iron (specific heat = 0.451 J/g °C) was placed in a beaker of 600. grams…

A: The question is about calculating the Original Temperature of the hot iron piece using the given…

Q: What is the change in the energy of surroundings when the system absorbs 17.5 kJ of energy and…

A: It is given that system absorbs 17.5 kJ of energy and the work done is 5×103 J. It is known that 1 J…

Q: The following two reactions are known: N2(g) + O2(g) -> 2NO(g) AH = +180.50 kJ N2(g) + 202(g) ---> A…

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Q: How much energy is required to change the temperature of 21.5 g Cu from 27.0 °C to 88.1 °C? The…

A: The weight of copper is 21.5 g. The given temperature values are 27.0 ˚C and 88.1 ˚C. The constant…

Q: In an experiment, 30.0 g of metal was heated to 98.0°C and then quickly transferred to 50.0 g of…

A: The heat capacity of the metal is to be calculated.

Q: Octane 1C8H182 is a liquid hydrocarbon at room temperature that is a constituent of gasoline.…

A: We have the equation ∆G°=∆H°-T∆S° Where ∆H° is change in enthalpy, ∆G° is change in free energy, T…

Q: A 237-g piece of iron, initially at 100.0 °C, is dropped into 244 g of water at 10.0 °C. When the…

A: The amount of heat required to increase the 1oC temperature of 1 g metal is known as the specific…

Q: Coffee cup calorimetry experiments can be used to obtain DHfo for magnesium oxide. To determine the…

A: The equation for the formation of magnesium oxide is given as: Mgs + 12O2g → MgOs Given: To…

Q: What is the work involved in a process where a system experiences a net loss of energy equal to 9.3…

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Q: Consider heating 1.0 kg of water at a constant pressure of 1 atm. How much heat is needed to raise…

A: Given : Mass of water = 1 kg = 1000g Pressure = 1 atm Initial temperature, t1 = 25°C Final…

Q: How much energy is lost when 50 g of iron cools from 45°C to 15°C? (specific heat capacity of iron =…

A: The relation between the amount of heat gained or lost (q) by a metal in a chemical process and the…

Q: When 1 mol of a fuel is burned at constant pressure, it produces 3455 kJ of heat and does 12 kJ of…

A: Delta E = q + w  where Delta E = change in internal energy  q = heat , w = workdone

Q: An unknown sample of coal is burned in an apparatus with a calorimeter constant of 1.62 kJ/°C. When…

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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…

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Q: Hydrogen gas, H2 , reacts explosively with gaseous chlorine, Cl2 , to form hydrogen chloride,…

A: Given, Hydrogen gas H2 reacts explosively with gaseous chlorine Cl2. What is the enthalpy of the…

Q: An 80.0 g sample of a gas was heated from 25 °C to 225 °C. During this process, 346 J of work was…

A: The relationship between the internal energy change, heat and work is given by  ΔE = q + W where ΔE…

Q: A substance is found to have a heat capacity of 400.0 J °C. How much heat (in kJ) is absorbed when…

A: Heat capacity is defined as the quantity of heat absorbed by substance to raise the temperature of…

Q: A system gains 20.4 J of internal energy while doing 30.0 J of work. Does heat enter or escape from…

A: From first Law of Thermodynamics , the total change in internal energy of the system can be…

Q: 4) Which of the following (with specific heat capacity provided) would show the smallest temperature…

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Q: An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.8 kJ/°C. When a…

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Q: 3.2 kJ of heat is added to a slug of silver weighing 38.5 grams. The heat capacity of the silver…

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Q: An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.75 kJ/°C. When…

A: Given:  Calorimeter constant(C)= 0.75 KJ/°C  Mass of sample(m) = 0.412 gm  Increase in temperature…

Q: III WICI a process occurs at constant external pressure. a) What is the sign of w for the system? Is…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: Calculate ΔE for a system that absorbs 506.0  kJ of heat from its surroundings and does 379.0  kJ of…

A: It is a given that a system absorbs 506 kJ of heat and the system does 379 kJ of work on the…