When 10.00 mL of 1.00 M HCl solution is mixed with 115 mL of 0.100 M NaOH solution in a constant-pressure calorimeter,the temperature rises from 22.45 °C to 23.25 °C. Calculate q for this reaction, assuming that the heat capacity of the calorimeteris the same as that of 125 g of water.9 =J A hot 120.8 g lump of an unknown substance initially at176.2 °C is placed in 35.0 mL of water initially at 25.0 °Cand the system is allowed to reach thermal equilibrium. Thefinal temperature of the system is 70.6 °C.Using this information and the specific heat values forseveral metals in the table, identify the unknownsubstance. Assume no heat is lost to the surroundings.titanium◇ graphitezincrhodiumaluminumtungstenSubstanceSpecific heat (J/(g∙°C))aluminum0.897graphite0.709rhodium0.243titanium0.523tungsten0.132zinc0.388water4.184

For No. 1: The amount of energy in the form of heat that is released by the hot lump of unknown…

Answered: When 10.00 mL of 1.00 M HCl solution is…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 11P

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How much heat is produced by combustion of 125 g of methanol under standard state conditions?
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