---### Calculating Enthalpy Change for a Neutralization ReactionIn a coffee-cup calorimeter, 120.0 mL of 1.4 M NaOH and 120.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 25.7°C. After the reaction, the final temperature is 31.0°C. Assuming that the solutions have a density of 1.06 g/mL and a specific heat capacity of 4.18 J/g∙°C, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.\[ \Delta H = \frac{\text{kJ}}{\text{mol}} \]---**Steps to Calculate Enthalpy Change (∆H):**1. **Measure Initial and Final Temperatures**: - Initial Temperature (Ti) = 25.7°C - Final Temperature (Tf) = 31.0°C2. **Calculate the Total Volume of Solution**: - Volume of NaOH solution = 120.0 mL - Volume of HCl solution = 120.0 mL - Total Volume = 120.0 mL + 120.0 mL = 240.0 mL3. **Determine the Total Mass of the Solution**: - Density of solution = 1.06 g/mL - Total Mass (m) = Total Volume * Density = 240.0 mL * 1.06 g/mL = 254.4 g4. **Find the Temperature Change (∆T)**: - ∆T = Tf - Ti = 31.0°C - 25.7°C = 5.3°C5. **Calculate the Heat Absorbed or Released (q)**: - Specific Heat Capacity (c) = 4.18 J/g∙°C - q = m * c * ∆T = 254.4 g * 4.18 J/g∙°C * 5.3°C = 5633.94 J (or 5.634 kJ)6. **Determine the Moles of Reactants**: - Volume of NaOH solution = 120.0

Volume of 1.4 M NaOH taken, V = 120.0 mL Volume of 1.4 M HCl taken, V = 120 mL

In a coffee-cup calorimeter, 120.0 mL of 1.4 M NaOH and 120.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 25.7°C. After the reaction, the final temperature is 35.1°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C-g, calculate the enthalpy change for the neutralization of HCI by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ = kJ/mol Submit Answer Try Another Version item attempt remaining

In a coffee-cup calorimeter, 120.0 mL of 1.4 M NaOH and 120.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 25.7°C. After the reaction, the final temperature is 35.1°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C-g, calculate the enthalpy change for the neutralization of HCI by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ = kJ/mol Submit Answer Try Another Version item attempt remaining

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 2.59 g sample of a substance suspected of being pure gold (Cs = 0.128 J g−1°C−1) is warmed to 81.3 °C and submerged into 14.8 g of water initially at 24.0 °C. The final temperature of the water and the gold is 26.9 °C. Assume that the specific heat capacity of water is 4.18 J g−1°C−1.What is the heat capacity of the unknown substance? Express your answer to 3 significant figures.
In an experiment, 28.0 g of metal was heated to 98.0°C and then quickly transferred to 150.0 g of water in a calorimeter. The initial temperature of the water was 24.5°C, and the final temperature after the addition of the metal was 32.5°C. Assume the calorimeter behaves ideally and does not absorb or release heat. What is the value of the specific heat capacity (in J/g•°C) of the metal?
In a coffee-cup calorimeter, 120.0 mL of 1.0 M NaOH and 120.0 mL of 1.0 M HCl are mixed. Both solutions were originally at 26.1°C. After the reaction, the final temperature is 32.8°C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
3. 50.0 mL of 1.0 M sodium hydroxide and 50.0 mL of 1.0 M hydrochloric acid, both at 22.5 °C, were mixed together in a calorimeter. The temperature increased to 29.2 °C. Determine enthalpy of the reaction. You may assume that both solutions have the same density and heat capacity of water (d = 1.00 g/mL, SH=4.184 J/g°C). Remember, AH = q at constant pressure.
In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 24.0°C. After the reaction, 3 the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ - kJ/mol
When 15.0 mL of 3.00 M NaOH was mixed in a calorimeter with 12.5 mL of 3.00 M HCl, both initially at room temperature (22.0 °C), the temperature increased to 29.0 °C. The resultant salt solution had a mass of 27.50 g and a specific heat capacity of 3.74 J K-1 g-1. What is the heat capacity of the calorimeter (in J/°C)? Note: the molar enthalpy of neutralization per mol is -55.84 kJ mol-1
[References] In a coffee-cup calorimeter, 100.0 mL of 1.3 M NaOH and 100.0 mL of 1.3 M HCl are mixed. Both solutions were originally at 24.3°C. After the reaction, the final temperature is 33.0°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C-g. calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. kJ/mol AH = Submit Answer Try Another Version 1 item attempt remaining 4 C C A 6 T
You mix 125 mL of 0.230 M with 50.0 mL of 0.575 M in a coffee-cup calorimeter, and the temperature of both solutions rises from 22.30 °C before mixing to 24.96 °C after the reaction. What is the enthalpy of reaction per mole of ? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g · K. Enthalpy of reaction = ?
An experiment was performed to calculate the heat of solution for potassium fluoride. Use the following data to determine its heat of solution. Assume that the specific heat capacity of the solution produced is the same as that of water, 4.184 J⁄g·°C. Identity of Salt KF Mass of water in calorimeter (g) 52.42 Mass of salt sample (g) 7.32 Initial temperature of Calorimeter (°C) 20.8 Final temperature of Calorimeter (°C) 30.3 Report your answer in kJ/mol to 3 significant figures.
If 35.0 g H2O at 22.7 °C is combined with 65.0 g H2O at 87.5 °C, what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.
3
When 1.091 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose, in kJ/mol?