What is the heat of a reaction, in joules, with a total reaction mixture volume of 68.8 mL if the reaction causes a temperature change of 5.1 °C in a calorimeter? Assume that the reaction mixture has a density of 1.00 g/mL and a specific heat of 4.184 J/g-°C. The calorimeter has a heat capacity of 10.0 J/°C. Type answer:

What is the heat of a reaction, in joules, with a total reaction mixture volume of 68.8 mL if the reaction causes a temperature change of 5.1 °C in a calorimeter? Assume that the reaction mixture has a density of 1.00 g/mL and a specific heat of 4.184 J/g-°C. The calorimeter has a heat capacity of 10.0 J/°C. Type answer:

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 11QAP: When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of...

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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?
A coffee cup calorimeter was calibrated using 5.01 mL of 0.901 M HCl and 10.01 mL of 0.751 M NaOH. Thereafter, T changed from 29.5oC to 32.5oC. Using the same calorimeter, the enthalpy of reaction between NaOH and HNO3 is determined by mixing 5.10 mL of 0.800 M HNO3 and 10.10 mL of 0.600 M NaOH. The T changed from 30.5oC to 32.5oC. Suppose that the delta H of reaction between H+ and OH- is -55.9 kJ/mol. i. Find the heat capacity of the calorimeter and the limiting reactant of the reaction studied. ii. Find qrxn and enthalpyexperimental of the reaction. iii. Find the % error.
Click the button within the activity, and analyze the relationship between the two reactions that are displayed. The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, ΔHΔH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2. Reaction 1: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g),C3H8(g)+5O2(g)→3CO2(g)+4H2O(g), ΔH1=−2043 kJΔH1=−2043 kJ Reaction 2: 5C3H8(g)+25O2(g)→15CO2(g)+20H2O(g),5C3H8(g)+25O2(g)→15CO2(g)+20H2O(g), ΔH2=?ΔH2=? Express your answer to four significant figures and include the appropriate units. View Available Hint(s)
Calculations for the Specidfic Heat for an Unknown Metal Trial 1 Trial 2 Mass of unknown metal(g) 18.371 18.371 Mass of calorimeter cup(g) 1.891 1.891 mass of calorimeter and water(g) 47.231 46.502 Tempature of boiling water bath (C) 98.50 99.2 Initial tempature of calorimeter water(C) 23.5 23.4 Final Tempature of water and metal(C) 24.8 24.8 Mass of water(g) Tempature change of water(C) (Do not include a negative sign) Heat gained by water (cal) (do not include negative sign) heat lost by metal(cal) (do not include negative sign) tempatire change of metal(C) (do not include negative sign) Specific heat of metal [cal/g. C] Specific heat of metal [J/(g. C)] Average specific heat of metal [J/(g·°C)] Identify the Metal based on the average specific heat in J/(g·°C)
When copper(II) sulfate pentahydrate (CuSO4·5 H2O) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor. The hydrated form is medium blue, and the dehydrated solid is light blue. The balanced equation is CuSO4·5 H2O(s) --> CuSO4(s) + 5 H2O(g) *heat above the arrow If 5.32 g CuSO4·5 H2O is decomposed to CuSO4, predict the mass of the remaining light blue solid.
Students were asked to determine the heat of reaction forthe neutralization of a newly synthesized monoprotic acid HX and NaOH. Theyfirst calibrated the styro ball calorimeter using the reaction of 15.0 mL of 0.100 MHCl and 20.0 mL of 0.0500 M KOH. This recorded a change in temperature from26.5 °C to 31.8 °C. Afterwards, they determined the heat of reaction for a mixtureof 5.00 mL, 1.00 M NaOH and 10.0 mL, 1.00 M HX. This showed an increase intemperature of 3.6 °C.i. What is the heat capacity of the calorimeter in J/℃ (∆? =-55.85??????????????kJ/mol)?ii. Write the balanced chemical and net ionic equations for the reaction of NaOHand HX .iii. What is the experimental enthalpy (in kJ/mol) for the neutralization reactionbetween HX and NaOH ?iv. Is the reaction between NaOH and HX endothermic or exothermic ?
Part B Consider the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l)C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 gg of sucrose, C12H22O11C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘CkJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C∘C. Calculate the change in internal energy, ΔEΔEDelta E, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.09g of glucose is burned in a calorimeter containing 826 g of water, and the temperature of the assembly increases from 20.10oC to 24.70oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol. (Final answer: TWO decimal places)
Give handwritten answer A coffee cup calorimeter is prepared, containing 100.000 g of water (specific heat capacity = 4.184 J/g K) at initial temperature 80.000 C. A salt weighing 7.308 g is quickly added. The salt has a molar mass of 178.051 g/mol. The final temperature of the solution is 51.028 C. Assume no heat loss to the surroundings. Assume the specific heat capacity of the solution is equal to that of pure water, and that the mass of the solution is equal to the mass of the solid plus the mass of water in the calorimeter. What is the molar heat of solution for the salt, in kJ/mol?
Chemistry Calculate the heat capacity of 2.00 L of water, given the specific heat of water is 4.187 kJ kg-1K-1. Calculate the percent difference between this value and the mean of the bomb calorimeter’s heat capacity of 10.00 KJ/K. Was the water a large contributor to the overall Cv?
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an important flavor component of vanilla extract is vanillin C8H8O3 molar mass = 152.15 g/mol when vanillin burns in a bomb calorimeter with a heat capacity of 8.60 kJ/°C the temp increases from 25.97°C to 31.18°C. if the heat of combustion of vanillin is -3760 kJ/mol what mass of vanillin (in g) was combusted? answer to two decimal places