A chemical system produces 170. kJ of heat and does 18 kJ of work. What is AE for the surroundings? O -152 kJ O 152 kJ O -188 kJ O 188 k.J

Q: A mixture of gases undergoes a chemical reaction inside of a container with a movable piston. The…

A: Here the heat is releases means it will be having a negative sign as q= -243KJ And here work is done…

Q: Which sample will reach the lowest final temperature when all samples evolve 12.5 J of heat and all…

A: Since, Q =m.c.St WHERE Q = heat energy M =mass of metal C= specific heat of metal Triangle T =…

Q: The specific heat capacity of silver is 0.24 J/°C·g. Calculate the energy required to raise the…

A: Heat capacity is an extensive property.  But specific heat capacity is intensive property.  Heat…

Q: 75.0 mL of 1.80 M CuSO 4 solution is mixed with 150 mL of 1.80 M NaOH solution in a coffee cup…

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Q: Consider the dissolution of CaCl2: CaCl2 (s) → Ca²+ (ag) +2 Cl¯(ag) AH=-81,5 kJ An 11.8-g sample of…

A: When a solute is dissolved in solvent to form a solution is called dissolution. It measures the…

Q: 3. When 1.010 g sucrose (C12H22011) undergoes combustion in a bomb calorimeter, the temperature…

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Q: Consider the following endothermic reaction: Which statement is true for the above reaction? OA.…

A: Answer:When energy gets released during the reaction then such reactions are called as exothermic…

Q: Consider the following reaction: 2 PbS (s) + 3 O2 (g) → 2 PbO (s) + 2 SO2 (g) AHxn = -827.4 kJ What…

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Q: A system does 467 kJ of work and loses 157 kJ of heat to the surroundings. What is the change in…

A: First law of thermodynamics It states states that heat is a form of energy, and thermodynamic…

Q: 7. For the following scenarios what is the metal? a. A piece of metal weighing 59.047 g was heated…

A: Given,a, mass of metal = 59.047 gInitial temperature of metal = 100.0 oCvolume of water = 100.0…

Q: A system does 521 kJ of work and loses 216 kJ of heat to the surroundings. What is the change in…

A: The objective of the question is to calculate the change in internal energy (ΔE) of a system that…

Q: 8. The equation for the combustion of methane, CH4 (the main component in natural gas) is shown…

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Q: Consider the dissolution of CaCl2: CaCl2 (s) → Ca+ (ag) + 2 Cl (aq) AH = -81.5 kJ An 11.8-g sample…

A: Calculate the heat released when 11.8 g of CaCl2 is dissolved:

Q: A system absorbs 21.6 kJ of heat while performing 6.9 kj of work on the surroundings. If the initial…

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Q: The specific heat capacity of a pure substance can be found by dividing the heat needed to change…

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Q: 26 kJ of work and loses 216 kJ of heat to the surroundings. ge in internal energy, AE, of the…

A: First law of thermodynamics is based on conservation of energy

Q: 4. A 505 gram piece of copper tubing is heated to 99.0 °C and placed in an insulated vessel…

A: Heat capacity: The amount of heat required to increase the temperature of a substance by one-degree…

Q: As a system increases in volume, it absorbs 52.0 J of energy in the form of heat from the…

A: Given: Decreased internal energy= 106.2 J Absorbed heat= 52.0 J Final volume= 58.6 L Working…

Q: The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of…

A: Heat capacity is the amount of heat required to raise the temperature of a substance by 10C.…