Answered: What would be the final temperature of…

What would be the final temperature of 231.6mL of NaCI solution upon releasing 24.1kJ of energy to the surroundings? Assume d = 1.02 g/mL; Cs = 4.184 J/g.°C; and the initial temperature is 50.0 °C.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 64QRT

See similar textbooks

Related questions

Q: ΔH = +572 kJ for the decomposition of water by the reaction 2 H2O() → 2 H2(g) + O2(g). How many…

Q: For the chemical reaction Ca (s) + ½ O₂ (g) → CaO (s) ∆H° = -635 kJ/mol. What is the molar enthalpy…

A: The balanced Chemical equation given in the question - Ca(s) + ½O₂(g) → CaO(s), ∆H° =-635 kJ/mol…

Q: Question 6

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

Q: When 1 g of material X(molar mass= 40/g/mol) was dissolved in a beaker containing 50.0 ml of 1 M HCI…

A: Given Mass of material= 1 g Molar mass of material = 40 g/mol Moles of material = mass of…

Q: When 8.6 grams of a certain compound is dissolved in 78 grams of water in a calorimeter, the…

Q: Given the following equation and the molar enthalpy of combustion of methane gas: CH4((g) +…

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: Sodium chloride, the table salt (NaCl) is added in cooking to enhance the flavor of the food. When…

A: specific heat capacity is defined as the amount of heat required to raise the temperature of a…

Q: Calculate the standard enthalpy change for the following reaction at 25 °C.…

A: If the reaction between the species acid and base than the salt and water will be generated.

Q: 07. Some instant ice packs contain ammonium chloride (NH,CI), which dissolves to produce two ions in…

Q: What is the Enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL…

A: Given : volume of solution = 250.0 mL density of solution = 1.25 g/mL and increase in temperature =…

Q: The standard molar enthalpy of formation of calcium carbonate (CaCO3) is - 1206.9 kJ/mol. What will…

A: (d) The reaction is as follows: CaCO3(s) → CaO(s) + CO2(g) The molar mass of CaCO3 = 100.1 g/mol…

Q: The standard enthalpy of reaction, AH' pxn, for the reaction, CaO(s) + SO3(3) – CaSO4(s) is -401.5…

Q: Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 20.9 g…

A: Given data : Molar mass of KNO3 (MK)= 101.1 g/mol Mass of KNO3 (mK) = 20.9 g Mass of water (mw) =…

Q: Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 34.4 g…

A: Given that: Mass of KNO3 = 34.4 g, mass of water = 217 g, initial temperature of water, Ti = 23.00⁰C…

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

Q: ΔH = +572 kJ for the decomposition of water by the reaction 2 H2O() → 2 H2(g) + O2(g). How many…

A: Number of moles decomposed = Heat given/Molar heat of decomposition Mass = Number of moles x molar…

Q: How much energy (at constant temperature and pressure) must be supplied as heat to 10.0 g of…

A: CL2 →10 gmmole=1071CL2→CI-+CI+1071mole 1071 1071

Q: When a 6.00 g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity…

A: We have to calculate the molar heat of solution.

Q: Consider the following chemical reaction: C3H4(g) + HCl (aq) ----------> C3H6Cl2(g) 412 kJ/ mole…

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

Q: Given the following equation and the molar enthalpy of combustion of methane gas:…

A: ∆H°comb of methane = -802.5 kJ Means, it is of one mole of methane. One Mole (16.04g) of methane…

Q: 3.61 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C.…

Q: A certain reaction has ∆?°= -19.5KJ and ∆S°= 42.7 J/K, is the reaction exothermic or endothermic?

Q: How much will the temperature of a 200g water at 95°C be reduced when a 45 g metal ( cp = 0.24 J/g…

A: The heat absorbed or released is given by : q = m. C. (T final - T initial ) Where q = heat…

Q: Energy Constants for H2O 334 J/g = Heat of Fusion (Hf) 2260 J/g = Heat of Vaporization (Hv) 2.11…

A: Answer:- This question is answer by using the simple concept of calorimetry which state that heat…

Q: When 4 grams of a certain compound is dissolved in 61 grams of water in a calorimeter, the…

Q: When 4.20 g of solid NH4NO3 dissolves in 50.0 g of water at 26.8°C in a calorimeter, the temperature…

A: The heat of a substance is given as:

Q: What is the change in temperature (in oC) when a 37 g sample of graphite (specific heat = 0.720 J/(g…

Q: Using the provided table, determine the molar enthalpy (in kJ/mol) for the reaction 2 K(s) + 2…

Q: When 1 g of material X(molar mass= 40/g/mol) was dissolved in a beaker containing 35.0 ml of 1 M HCI…

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

Q: Define standard enthalpy of formation (AH°;).

A: To define: standard enthalpy of formation.

Q: Determine the total heat absorbed by the reaction, in kJ, if 2.50 g of O, is required to fully…

Q: When 15.8 g KBr(s) dissolves in 119.7 g of water at 24.2°C, the final temperature of the solution…

Q: The standard enthalpy of reaction, AH rxn, for the reaction, CaO(s) + SO3(g) → CaSO4(s) is -401.5 kJ…

A: Mole can be defined as a standard unit for measuring large quantities of very small entities such as…

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: 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: 6. The autoionization constant of water (Kw) has a value of 2.00 x 10-14 at 25.0°C. This value…

A: Autoionization of water is the self ionization of water to produce H3O+ and OH- ions.The equation is…

Q: 2. When 100.0 mL of a 1.50 M HCl solution is combined with 60.0 mL of a 3.00 M LiOH solution the…

A: Given : Volume of HCl = 100.0 ml = 0.100 L Concentration of HCl = 1.50 M Volume of LiOH = 60.0 ml…

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

A: The enthalpy change during dissolution is equal to the heat absorbed by the solution.…

Q: The standard enthalpy change for the following reaction is 450 kJ at 298 K Cu(OH)2(s) → Cu(s) +…

A: Given:

Q: The reaction of 10.0 mL of 0.125 M NaOH and 5.0 mL of 0.500 M HNO3 gives a temperature rise of 1.36…

A: Answer: Acid and base neutralization reaction is an exothermic reaction and heat of neutralization…

Q: 15. The enthalpy change CH,(g) + 20,(g) → CO,(g) + 2H,O(1) breams is -891 kJ for the reaction as…

A: Given :

Q: Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 48.7 g…

Q: Using the provided table, determine the enthalpy for the reaction 2 K(s) + 2 H,O(1) → 2 KOH (aq)…

A: The chemical reaction is:2 K (s)+ 2H2O (l) → 2KOH (aq)+H2 (g) ∆HrGiven: ∆Hf° {K (s)} = 0∆Hf°…

Q: 18b. Calculate the standard enthalpy change, AHU, for this reaction using section 12 of the data…

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…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

What would be the final temperature of 231.6mL of NaCI solution upon releasing 24.1kJ of energy to the
surroundings? Assume d = 1.02 g/mL; Cs = 4.184 J/g.°C; and the initial temperature is 50.0 °C.

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 Formula

Step 2 Given

Step 3 Calculations

Step 4 The answer

Step by step

Solved in 4 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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.
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.)
Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4 °C causes the temperature to rise to 25.8 °C. What is the approximate amount of heat involved in the dissolution, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?
In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Define the joule in terms of SI base units.
Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?
Magnesium sulfate (MgSO4) has a solubility of 38.9 g/ 100 g H2O at 30C. A solution is prepared by adding 9.50 g of MgSO4 to 25.0 g of water at 40C. A homogeneous mixture is obtained. Is the solution saturated, unsaturated, or supersaturated? One gram of magnesium sulfate is added to the solution cooled to 30C. Would you expect some of the MgSO4 to precipitate? If so, how much? If not, how much more MgSO4 can be added before precipitation takes place?
A 0.500-g sample of KCl is added to 50.0 g of water in a calorimeter (Figure 5.12). If the temperature decreases by 1.05 °C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?
9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?
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?
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?
Convert the units of Henrys law constant for CO2, in table 7.2, to units of, mmHg, atm, and bar. In which cases does the numerical value of the constant change?