A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 23.5 degrees (C)  before mixing and 31.0 degrees(C)  after mixing. The heat capacity of the calorimeter is 12.1 J/K.  From these data, calculate ΔH for the process: CuSO4(1M)+ 2KOH(2M) →Cu(OH)2(s) + K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.

Q: In a constant‑pressure calorimeter, 65.0 mL of 0.350 M Ba(OH)2 was added to 65.0 mL of 0.700 M HCl.…

A: Given:65.0 mL of 0.350 M Ba(OH)265.0 mL of 0.700 M HCl.Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O

Q: Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon…

A: According to Hess’s law of constant heat summation, the total enthalpy change for a reaction is the…

Q: Determine the mass of CO2CO2 produced by burning enough carbon (in the form of charcoal) to produce…

A: The balanced chemical reaction is  C(s)+O2 (g)→CO2(g); ΔrH∘=−393.5 kJ-mol-1  The mass of CO2…

Q: If we measure the heat change (q) of everything in a system except the calorimeter, we can use the…

A: Hot water will lose it and cold water and the calorimeter will gain heat.

Q: When 14.7 g of CaCl2(s) (molar mass 111.0 g/mol) was dissolved in water in a constant pressure…

A: We have 14.7 g of CaCl2 dissolved in water in a constant pressure with heat capacity 1168J/°C The…

Q: A 5.00 grams of LiOH is dissolved in 100.0 grams of water in a perfect calorimeter. Calculate the…

A: Given data,  Mass of LiOH = 5.00 g  Mass of water = 100.0 g  LiOH(s) --> Li+(aq) + OH-(aq) , ∆H…

Q: When a 4.25-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup…

A: Given,Mass of sample = 4.25-gInitial temperature = 22 degree CelsiusFinal temperature = 16.9 degree…

Q: ΔH for the dissolving process KOH (s) → KOH (aq) is -57.6 kJ/mol KOH.  In an insulated calorimeter,…

A: In calorie meter we can calculate the hate of the reaction .

Q: From experiments, you know the following thermochemical equations: CaO(s) + 2HCl(aq) ---> CaCl2(aq)…

A: Given: CaO(s)+2HCl(aq)→CaCl2(aq)+H2O(l)       ∆H1=-186 kJ ---eqn(1)CaO(s)+H2O(l)→Ca(OH)2(s)…

Q: When a 3.91 g sample of solid sodium hydroxide was dissolved in a calorimeter in 110.0 g  of water,…

A:

Q: 148 g sample of solid LiI-3H₂O (s) is dissolved in 212 mL of water in a coffee cup calorimeter. Once…

A: Givenmass of LiI.3H2O = 148 g Volume of water = 212 mL Final temperature= 18.69°C We have to find…

Q: If a system has 475 kcal475 kcal of work done to it, and releases 5.00×102 kJ5.00×102 kJ of heat…

A:

Q: aq) with 25.00 mL of 2.56 M HCl(aq). If the temperature changed from 25.0 Degree C to 38.4 degree C,…

A: Introduction Generally the heat released in the reaction is absorbed by the solution and raises the…

Q: When 5.40 g of a solid mixture composed of NH4Cl and CaCl2 was dissolved in 100.0 mL of water, the…

A: Given Mass of NH4Cl = 1.78 g Mass of CaCl2 = 3.26 g

Q: Energy change is the sum of heat and work:  ΔE = q + w.  Work is calculated by: w = -PΔV What is…

A: Given, a reaction absorbs heat =40.3 J =+40.3 J and volume of gas increases from 0.250 L to 0.750…

Q: When 1.045 g of CaO is added to 50.0 mL of water at 25.0 ∘C in a calorimeter, the temperature of the…

A:

Q: Two pollutants that form in auto exhaust are CO and NO. An environmental chemist must convert these…

A: The question is based on the concept of Hess's law.   It states that the net enthalpy change during…

Q: A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HCl in a calorimeter.…

A:

Q: Consider the following reaction: 2 Mg(s) + O2(g) ⟶⟶ 2 MgO(s)…

A: There is a  the  reaction  :- 2 Mg(s) + O2(g) ------------> 2 MgO(s).…

Q: oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC,…

A: Heat(q) = m.c..□T Using energy conservation,  Heat loss by Acid = Heat gain by water + Calorimeter…

Q: If a system has 225 kcal225 kcal of work done to it, and releases 5.00×102 kJ5.00×102 kJ of heat…

A: Given, w = 225 kcal q = - 5.00*102 KJ The negative sign indicates the energy is released by the…

Q: THERMODYNAMICS: A 1.16 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb…

A:

Q: When 1.045 g of K2O is added to 50.0 mL of water at 25.0 ∘C in a calorimeter, the temperature of the…

A: Information of question

Q: 1.22 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The…

A:

Q: A piece of metal weighing  5.10 gg   at a temperature of  48.5 ∘C∘C   was placed in a calorimeter in…

A:

Q: THERMODYNAMICS: A 1.98 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb…

A: Given the mass of acetic acid (HC2H3O2) sample taken = 1.98 g Since the temperature of the…

Q: 5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the…

A: The question can be solved by giveb formula,  Q=m×C×dT where Q = heat energy (Joules, J),  m = mass…

Q: A 1.66 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The…

A:

Q: When 0.418 gg of pentene, C5H12C5H12, is burned in a bomb calorimeter the temperature rises by…

A: The objective of this question is to calculate the combustion energy (ΔE) for pentene, C5H12, when…

Q: Write the balanced equation (total ionic) for the

A: We haven to give the total Ionic equation of given reaction, and tell why reaction got heated up.…

Q: When 1.045 g of CaO is added to 50.0 mL of water at 25.0 PC in a calorimeter, the temperature of the…

A:

Q: Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and…

A:

Q: 1.) The internal energy of a system increases 253 J , while the system loses 93 J of heat.…

A: Internal energy (∆E) :-         It is the energy of a thermodynamic system which is present in that…

Q: 1.87 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The…

A: Mass of acetic acid = 1.87g Molar mass of Acetic acid = 60g/mol Heat capacity of calorimeter =…

Q: A quantity of 2.00 ×102 mL of 0.715 M HCl is mixed with 2.00 × 102 mL of 0.358 M Ba(OH)2 in a…

A: Molarity - ratio of number of moles of solute to the volume of solution in litres. Formula is,…

Q: 150 mL of a 0.728 M HCl aqueous solution is mixed with 150 mL of 0.364 M Ba(OH)2 aqueous solution in…

A: Answer:This question is based on the principle of energy conservation where energy lost during the…

Q: A 1.79 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The…

A:

Q: Consider the following reaction:   2 HCl(aq) + Ba(OH)2(aq)  ⟶⟶ BaCl2(aq) + 2 H2O(l)          ΔH=…

A: When the acid and base that is one equivalent to both of the components undergoes neutralization…

Q: Calculate the change in internal energy (ΔU) for a system that is giving off 25.0 kJ of heat and is…

A: The first law of thermodynamics states that the change in internal energy of a system equals the net…

Q: A 25g of CaCl2 is dissolved in 250ml of water in a coffee-cup calorimeter.  The temperature of…

A:

Q: Which of the following is a statement of Hess's law?     If a reaction is carried out in a series of…

A: Thermodynamics is branch of chemistry in which we deal with amount of heat absorbed or evolved…

Q: A 2.673 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of…

A: Tf = 28.80°C  Ti = 25.03° C ΔT = Tf - Ti = 28.80° C - 25.03 ° C                                =…

Q: A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic…

A: Given weight of Zn = 2.50 g [HBr] = 2M Volume of HBr = 100mL= 0.1 L No. Of moles of HBr = 2 x 0.1 =…

Q: What is the final temperature of a system if 11.00 g of gold at 90.0°C is placed in 11.00 g of water…

A:

Q: THERMODYNAMICS: A 1.42 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb…

A:

Q: If we measure the heat change (q) of everything in a system except the calorimeter, we can use the…

A: Given: mass of hot water = 5.59 g mass of cold water = 5.62 g C = 4.186 J/g°C Temperature of hot…

Q: THERMODYNAMICS: A 1.87 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb…

A: