A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 71 J of heat while 35 J of work is done on it. Step 2: The system absorbs 35 J of heat while performing 71 J of work. Calculate ΔE for the overall process. ΔE = _____J

Q: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 71 J…

A: The relationship between the parameters is given as where w = work and q = heat

Q: A system undergoes a process consisting of the following two steps:Step 1: The system absorbs 72 J…

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Q: 226 kJ of heat increases the temperature of 47.0 kg of copper by 12.5 ℃, what is the molar heat…

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Q: 100 J of heat is released by the system and it does 100J of work. Which of the following is true? A.…

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Q: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 72 J…

A: Please have a look on the solution attached below

Q: If 1.42 kcal of energy is required to raise the temperature of a 190 g sample of pure iron, by how…

A: Q - heat = 1.42 Kcal m - mass = 190 g C - specific heat =0.45 J/g-°C ΔT - change/rise in temperature…

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Q: A sample of liquid absorbs 13.5 kJ of heat and does 1.8 kJ of work when it vaporizes. Calculate ∆E…

A: Given that : Heat absorbed by the sample (Q) = +13.5 kJ Work done (W) = 1.8 kJ

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Q: on 25 « < Questio 4 points onsider the following metals and their specific heat capacities. If the…

A: We know Q= ms∆t    , Q= amount of  heat absorbed., m =mass.,  s = specific heat capacity , t =…

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A: Heat released by a system has a negative sign and work done on the system has a positive sign.

Q: The change in internal energy of a system is +10.0 J and the system acquires 15 J of heat. How much…

A:

Q: How much energy is absorbed during the complete reaction of 233.0 g calcium oxide (MW = 56.08 g/mol)…

A: First convert the given mass of CaO into moles. Moles=MassMolar mass=233.0g56.08 g/mol=4.155 mol

Q: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 69 J…

A: Given data,Step 1:Heat(Q)=69JWork(w)=-34J(-ve sign represent work is done on the system)Step…

Q: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 68 J…

A: The process happening on the system is of two steps given as,

Q: Calculate the amount of heat released by a given reaction, causing the temperature of 500 mL water…

A: Volume of water = 500 ml Density of water = 1 g/ml Change in temperature = 5.2 ℃  Specific Heat of…

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: Consider the reaction: When a 10.0-g sample of ethyl alcohol (molar mass = 46.07 g/mol) is…

A: The given reaction is : C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l)        ∆H=-1.37×103 kJ

Q: energy (in joules) is needed to heat 200.0 g of water by 10.0 C? The heat capacity of water is…

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Q: A system undergoes a process consisting of the following two steps:Step 1:The system absorbs 72 J of…

A: The question is based on the concept of chemical thermodynamics. We have to calculate internal…

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: 46.0 g of a mercury alloy is heated from 20.0°C to 105.°C, and absorbs 550. joules of heat in the…

A: q = mc∆T  q is heat , m is Mass , c is specific heat capacity , ∆T is the difference in temperature…

Q: What is the change in internal energy for a system that performs 213 kJ of work on its surroundings…

A: Given, System performs 213 KJ of work on its surrounding And system loses 79 KJ of heat in the…

Q: A cylinder contains a gas under constant atmospheric pressure. When 0.434 kJ of heat is added to the…

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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: 220 g quantity of a certain metal is heated to 100.0 °C. The metal was immediately immersed into 258…

A: The question is based on the concept of specific heat capacity. it is defined as the amount of heat…

Q: If 250. g of aluminum is consumed in the reaction, how much heat (in kJ) could theoretically be…

A: 2 Al (s) + Fe2O3 (s) → 2 Fe (l) + Al2O3 (l)              ΔH = −848.0 kJ In the given reaction there…

Q: Which of the following would show the largest temperature change upon gaining 200 J of heat? (s is…

A: The heat is given as the following formula: Q=m×specific heat capacity×∆TQ=Heatm=mass of…

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

A:

Q: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 75 J…

A: The process happening on the system is of two steps given as, Step 1: The system absorbs 75 J of…

Q: (1) Calculate (a) q when a system does 54 J of work and its energy decreases by 72 J. (b) DE for…

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Q: A metal weighing 45.6g loses 350.6J of heat when it’s temperature is lowered from 89.2oC to 64.2o…

A:

Q: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 71 J…

A:

Q: What is the change in internal energy for a system if the system absorbs 322 kJ of heat and has…

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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: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 75 J…

A:

Q: & How much work is done by or on the system (state which), in kcal, in a reaction if the internal…

A: Given: Mass of water = 185 g. Initial temperature of water = 20.0 oC Final temperature of water =…

Q: absorbs 1.357E3 J of heat. The final temperature of the sand is 6.7E1 °C. What is the mass (in g) of…

A: Given: Initial temperature = 2.24E1 °C Final temperature = 6.7E1 °C Amount of heat absorbed =…

Q: What is the ΔE for a system which has the following two steps: Step 1: The system absorbs 60 J of…

A: We are given with heat absorbed or released and the work is done on or by the system which proceeds…

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Q: A chemical system produces 170. kJ of heat and does 18 kJ of work. What is AE for the surroundings?…

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Q: Consider the following reaction: 2Mg(s)+O2(g)⟶2MgO(s)ΔH∘=−1203kJ What mass of magnesium must be…

A: Magnesium reacts with oxygen to form magnesium oxide. The equation for the balanced chemical…

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: Given data, Work done = 346 J Mass of the sample = 80 g Internal energy increased by 7115 J

Q: If a system produces 135.0 kJ of heat and does 45.0 kJ of work on the surroundings, what is the ∆E…

A: The first law of thermodynamics is mathematically expressed as: ∆E=Q+W ...........................…

Q: In a certain process, 400 J of heat is added to a system and the system simultaneously does 100 J of…

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Q: The combustion of propane is represented by the following reaction: 50 21g) 3CO2(8) 4H2O(g) 2043 kJ…

A: The balanced reaction taking place is given as, =&gt; C3H8 (g) + 5 O2 (g) ---------&gt; 3 CO2 (g) +…

Q: If a system has a change in energy of 400 J and produces 200 J of work, how much heat was added to…

A: According the the first law of thermodynamics,  ∆U = q + w  Where : ∆U = internal energy  q = heat…

Q: Which of the following best defines molar heat capacity. a. The quantity of heat required to raise…

A: heat capacity is the property of matter which is the amount of heat required to raise the unit…

Q: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 74 J…

A: We have given that a system undergoing a process consisting of two given steps. And asked for the ∆E…