An experiment was conducted to find the heat of neutralisation in an acid - basereaction.A solution was madeby dissolving 3.79g of barium hydroxide in 100 mL of water. 30.0 mL of this barium hydroxide solution wasreacted with 27.0 mL of a 0.400 mol L-1solution of nitric acid. The heat of neutralisation was calculated to be51.7 kJ mol-1. Calculate the temperature change and the resultant pH of the solution

Approach to solving the question:q=mcΔT558.36 J=57.0 g×4.18 J/g°C×Δ𝑇558.36 J=57.0 g×4.18…

Answered: An experiment was conducted to find the…

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...

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A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol
If the heat of precipitation of barium sulfate is -1473.2 kJ/mol, what is the heat of solution (barium sulfate dissolving in water) of barium sulfate? Heat of precipitation: Ba2+(aq) + SO42-(aq) → Ba(SO4) (s) ΔH = - 1473.2 kJ/mol
when 3 L of silver nitrate and 3 L of hydrochloric acid, both at 0.25 M, are mixed, a precipitate is formed. The enthalpy change for the reaction is -45 J. Calculate the enthalpy change in kJ/mol of silver chloride.
How many mole is present in the reactant and product in the given belwo
Part b For the reaction given in Part A, how much heat is absorbed when 2.60 mol of A reacts? And part c said At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?
4. (a) Use the total solution volume, density of water, measured temperature change, and specific heat of water to calculate the heat absorbed by a solution (q soln) mixed in the proportions described by the response regulations. (b) Calculate the amount of heat that would be released during an acid-base neutralization reaction (qneut) like the one described in the response regulations. (c) Calculate the number of moles of H and OH initially present and the number of moles of H2O produced in the response regulation reaction
The heat of solution of a solid sample was determined using a coffee cup calorimeter that contains 250 milliliters of water initially at 25°C. As the sample is dissolved in the water, the temperature of the water decreased to 11°C. What is the heat of solution of the sample? Assume that the density of water is 1.00 g/ml and that the coffee cup is a good insulator. How much heat is released by a 96 gram piece of copper as it cools from 450°C to 48°C.
During an experiment, a student calculated the heat of neutralization reaction to be - 52.8 kj/mol. But when he checked the Handbook of Chemistry, he found that the standard AH of neutralization as - 59.5 kj/mol. What is the percent error in his calculation? 11.26 % Oa. O b. 88.74 % Oc. 12.69 % O d. 87.31 % 0.113 % Oe.
How much heat is released when an excess of Fe reacts with 48 g of 02 (M = 32 g/mol), according to the following reaction: 4Fe(s) + 302(8) → 2Fe,O3(s) AH = -1652 kJ 826 kJ O 1041 kJ O 2478 kJ O 1652 KJ
A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup calorimeter fitted with a lid through which a thermometer passes. The acid-base reaction is as follows: 2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(ℓ) The temperature of each solution before mixing is 22.3 °C. After mixing, the temperature of the solution mixture reaches a maximum temperature of 31.4 °C. Assume the density of the solution mixture is 1.00 g/mL, its specific heat is 4.18 J/g⋅°C, and no heat is lost to the surroundings. Calculate the enthalpy change, in kJ, per mole of H2SO4 in the reaction. +85.6 kJ/mol ‒85.6 kJ/mol +5.71 kJ/mol ‒5.71 kJ/mol ‒114 kJ/mol
In a coffee cup calorimeter with a heat capacity of 21.5 J/ºC, 225 mL of 0.20 M KOH at 22.3 ºC neutralizes 225 mL of 0.20 M HCl at 22.3 ºC. After the reaction occurs, the temperature of the resulting mixture is 29.2 ºC. The density of the final solution is 1.00 g/mL and the specific heat is 4.18 J/g°C. Calculate the Heat of neutralization of KOH.
Calculate the % yield when you react 20 mg of KBrO3 and produce 5 mg of KBr, assume all other reagents are in excess. Balance the equation, indicate the reactants and the products. (KBrO3 Molecular mass: 166.999 g/mol, KBr Molecular Mass: 119.002 g/mol) KBrO3 + Kl + HBr ➞ KBr + H2Oc. If the reaction produce ΔH= -2456kj. Is the reaction endothermic or exothermic? d. How many atoms of Oxygen are in 20mg of KBrO3?

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