A 75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC. Then the reaction is proceeded and the final temperature is reached to 28.000 oC. Calculate the heat of reaction in kJ / mole.

A 75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC. Then the reaction is proceeded and the final temperature is reached to 28.000 oC. Calculate the heat of reaction in kJ / mole.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

See similar textbooks

Related questions

Q: 75.0 mL. of 2.00 MHCl(aq) at 22.0 oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 oC. Then…

Q: Question 6

A: For the given process, the heat change may be calculated as:

Q: 13.6 g of solid ammonium nitrate (NH4NO3, molar mass 80.052 g/mol) is dissolved in 120 mL of water.…

A: Heat of solution is Calculated using formula: ∆Hsolution = - q / n Where , q = heat of solution…

Q: From the solutions above which ones are exothermic and which oness are endothermic? And what are the…

A: Exothermic reactions are reactions or processes that release energy, usually in the form of heat,…

Q: 8. If the accepted value for the heat of solution for NH,NO, is 25.69 kJ/mol, calculate the percent…

A: Molar enthalpy of solution is the amount of heat released or absorbed per mole of a substance. It is…

Q: 25 ml of 1M HCI la0) at 23.4°C was added to 25 ml of 1M NAOH at 23.4'C. The final temperature of the…

Q: In a calorimeter experiment, NaOH and HNO3 underwent a neutralization reaction and produced…

A: Neutralization reactions are generally exothermic and thus ΔH is negative.

Q: A tablespoon (about 15.0 mL) of sodium chloride, a common table salt, is dissolved in water. What is…

A: Given :- Volume = 15ml density of NaCl = 2.16 g/cm3 Delta H = 3.87 KJ/mol

Q: The Gibbs free energy of formation at 298K and 760 torr for ZnS(s), ZnO(s), and SO2(g) are: -48.11,…

Q: When 1.3 g of KClO3 was added to 151.1 g of water in a calorimeter, the temperature dropped by 0.588…

A: Given, Mass of KClO3= 1.3g Mass of water= 151.1g Temperature dropped(dT)=0.588°C The heat capacity…

Q: What is the dH, in kJ/mol, for the precipitation of AgCl if adding 125 mL of 1.00 M AgNO3 to 125 mL…

Q: Please answer completely with formula, given and complete solution so that i will understand. Tyms❤️…

A: In coffee cup calorimeter heat of reaction is given below. qrxn=-m×Cs×(Tf-Ti) Where m is mass of…

Q: In a reaction between Na and HCl, when 0.560g of Na is added to 75.0mL of HCl, the temperature rose…

A: Since you have posted questions with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: . Find the maximum possible temperature that may bereached when 0.050 mol Ca(OH)2(s) is allowed to…

A: Number of moles of strong acid HCl = 1 mol Number of moles of strong base Ca(OH)2 = 0.05 mol 1 mol…

Q: 6.41 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C.…

Q: When 375.0g of iron block is 87C was added to water at 15C, the system reached 33C. What mass of…

A: The energy of a system always remains the same. It is only transferred from one substance to…

Q: Calculate the enthalpy of solution for the dissolution of lithium iodide, LiI, molar mass = 133.85 g…

Q: . Calculate the change in the temperature of the solution.

A: The heat of dissolution is absorbed by solution to raise its temperature. As the solution is…

Q: When 30.0 mL of 0.400 M Ca(NO3)2 is added to 30.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in…

A: Given : Volume of Ca(NO3)2 = 30.0 ml Molar concentration of Ca(NO3)2 = 0.400 M Volume of NaF =…

Q: Using thermodynamic data given below, calculate the Gibbs free energy change, ΔG°rxn for the…

A: Given reaction Fe (s) + 2HCl (g) → FeCl2 (s) + H2 (g) Molecule/atom ΔGf°(kJ/mol) Fe 0 FeCl2…

Q: The standard nthalpy of neutralization of a weak hydrogen cyanide acid, HCN (aq), by a stong base,…

A: Since the standard enthalpy of neutralisation of part A (i.e strong acid and strong base ) = -60.066…

Q: The salt potassium perchlorate is soluble in water. When 2.84 g of KClO4 is dissolved in 106.00 g of…

A: Mass of KClO4 = 2.84 g Mass of H2O = 106 g Total mass of mixture = (106 + 2.84) g Temperature…

Q: The density of all solutions are 1.0g/mL and their respective heat capacities 4.184J/g.K.…

A: The heat of reaction qr can be calculated by this general formula Q = mC (change in temperature)…

Q: 4.51 g of MgSO, is placed into 100.0 mL of water. The water's temperature increases by 6.70°C.…

Q: 0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's…

Q: precipitation reaction. A 50.0 ml. solution of 0.330 M AGNO, was mixed with 50.0 ml. of 0.170 M KI.…

A: From the given data we haveTotal volume of solution=50+50=100mldensity of the solutions=1g/mLSo…

Q: What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 3 O2 (g) ⇌ 2 O3 (g) The…

A: Standard Gibbs free energy of formation of O2(g), ∆Gfo(O2, g) = 0.00 kJ.mol-1 Standard Gibbs free…

Q: Chlorhexidine gluconate Purified water q.s. Make a solution such that 1 tsp diluted to 1 gallon with…

A: a. The solution is 1:4200 w/v solution.

Q: Calculate the standard enthalpy change for the following reaction at 25 °C. MgCl, (s) + H,O(1)…

Q: Calculate the standard enthalpy of reaction, Δ?∘rxn,, of each of the given acid–base neutralization…

A: since there are more than three sub-parts, we are authorised to answer only the first three sub…

Q: ute solution of hydrochloric acid with a mass of 606.87 g and containing 0.31625 mol of HCl was…

Q: Calculate the heat generated by a reaction mixture of 8.4 L of sulfur dioxide at 1.00 atm and 273 K…

A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…

Q: The molar enthalpy change for the neutralization reaction: HCl(aq)+NaOH(aq)⟶NaCl(aq)+H2O(l) is ΔrH°…

Q: What is the change in enthalpy in joules when 5.44 x 10- mol of AgCI dissolves in water according to…

A: Given Reaction: AgCl--------> Ag+ +Cl- Moles of AgCl = 5.44 x 10-4 mol Δ H=65.5 kJ

Q: 5.21 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C.…

A: In order to increase one unit temperature of a substance, the amount of energy supplied in the form…

Q: ml of 1M HCI (ag) at 23.4'C was added to 25 25 ml of 1M NAOH at 23.4°C. The final temperature of the…

Q: A student followed the procedure in this experiment, using 29.5 mL of 1.59 molar HCl and 31.0 mL of…

Q: 11. When a 1.0 g of material X (molar mass = 40 g/mol) was dissolved in beaker containing 50.0 g of…

A: Given: Mass of X = 1 g Molar mass of X = 40 g/mol

Q: What is the change in enthalpy in joules when 5.44 x 10 mol of AgC dissolves in water according to…

A: The given chemical reaction is as follows,AgCl(aq) →Ag+(aq)+Cl-(aq) ; ∆H =65.5 kJnumber of moles…

Q: The following thermodynamics data were obtained for dissolving KNO3 in water: The slope of the…

A: The equation that relates equilibrium constant and Gibb's free energy is; ∆Go=-RT ln…

Q: The salt sodium perchlorate is soluble in water. When 8.44 g of NaClO4 is dissolved in 104.00 g of…

A: Given that : Mass of NaClO4 (mn)= 8.44 g Mass of water (mw) = 104.00 g Change in temperature ∆T=…

Q: A reaction is carried out at 25 °C with AH° = 20 kcal/mol and AS° = 25 cal/K-mol. (R : 8,314 J/K-mol…

Q: Calculate the heat of reaction per mole of water if addition of 25.0 mL of 0.101 M A H2SO4 to 50.0…

A: given molarity of H2SO4 = 0.101 M molarity of NaOH = 0.103 M volume of H2SO4 = 25ml volume of NaOH…

Q: At 25°C, the standard enthalpy of formation of HF(aq) is -319.9 kJ/mol. Of OH (aq), it is -229.5…

Q: 81.6 g of a metal alloy was heated to 93 o C, then plunged into 105 mL of H 2O that was at 19.5 o C.…

Q: .When solutions of an acid and a base are mixed, heat is released. Using a coffee-cup calorimeter,…

A: The reaction taking place is given as, => NaOH (aq) + HCl (aq) ⇔ NaCl (aq) + H2O (l) Given:…

Q: 4.71 g of M9SO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C.…

A: Since the temperature of water is increased, heat is released by the dissolution reaction of…

Q: 4.06 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C.…

A: Enthalpy of reaction is determine by change in enthalpy of product and reactant. Enthalpy of…

Q: 5.61 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C.…

A: To increase one unit of temperature of a subsyance. The amount of energy supplied in the form of…

Question

A 75.0 mL. of 2.00 MHCl(aq) at 22.0 ^oC is added to 150.0 mL. of 0.300 M NaOH(aq) at 22.000 ^oC. Then the reaction is proceeded and the final temperature is reached to 28.000 ^oC. Calculate the heat of reaction in kJ / mole.

Hint: Treat this mixture as a diluted solution.

C_P of H₂O(l) = 4.184 J / g ^oC

D of H₂O = 0.988 g/ mL.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
ou place hot metal into a beaker of cold water. ol type='a'> Eventually what is true about the temperature of the metal compared to that of the water? Explain why this is true. i>Label this process as endothermic or exothermic if we consider the system to be the metal. Explain. the water. Explain.
Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25C contains 15.0 mL of water at 25C. A 2.00-g sample of MgSO4 is dissolved in the water and 1.51 kJ of heat are evolved. (You can make the following assumptions about the solution: volume=15.0 mL, density=1.00 g/mL, specific heat=4.18J/gC.) (a) Write a balanced equation for the solution process. (b) Is the process exothermic? (c) What is qH2O? (d) What is the final temperature of the solution? (e) What are the initial and final temperatures in F?
The answer to the question in the picture is 217 kJ. For the reaction given in Part A, ΔS∘rxnΔSrxn∘ is 25.0 J/KJ/K . What is the standard Gibbs free energy of the reaction, ΔG∘rxnΔGrxn∘?
1. Write and balance the chemical equation where KOH and HCL reacts. 2. calculate ΔHb for the reaction involving K with HCl. Report your value in units of kJ/mole. 3. Calculate ΔH for the reaction involving MgO and HC1. KOH (s) + HCl (aq) → KCl (aq) + H2O (I) ΔH=
When 375.0g of iron block is 87C was added to water at 15C, the system reached 33C. What mass of water was used? Assume no heat loss.
The quantity of 83.0 g of potassium iodide (KI) is added to water to give a solution with a mass of 150. g. Assume that this solution is very dilute and thus has the same heat capacity as water. The dissolution reaction and the associated heat for potassium iodide is KI (s) -→ K+(aq) + I-(aq) qrx = DHrx = +20.3 kJ. Calculate the change in the temperature of the solution.
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 63.5 mL water (where X is a hypothetical metal): X + 2 HCl → XCl2 + H2 In this process, the water temperature rose from 25.0 °C to 34.1 °C. If 0.00618 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1 Express in 2 sig digs!
A 5.00 g-sample of KOH at 25.0 C was added to 100.0 g of H2O(l) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH is a thermodynamically favorable process? A. The forces between the ions and the water molecules are stronger than the forces between water molecules, thus, delta H < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus delta S > 0. Therefore, delta G < 0. B. The energy require to break the bonds between the ions in the solid is less than that released as the ion-dipole attractions form during solvation, thus delta H < 0. Also, the ions become widely dispersed as KOH(s) dissolved, thus delta S > 0. Therefore, delta G < 0. C. The average kinetic energy of the particles increases, resulting in delta H > 0. Also, the…
Calculate the enthalpy of solution for the dissolution of lithium iodide, LiI, molar mass = 133.85 g mol-1. When 1.49 g of LiI is dissolved in a coffee cup calorimeter containing 75.0 mL of water the temperature increased from 23.5 °C to 25.7 °C. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1. -62 kJ mol-1 -39 kJ mol-1 30 kJ mol-1 -76 kJ mol-1 18 kJ mol-1