THERMOCHEMISTRY237233. A student wishes to determine the enthalpy of the reaction of hydrogen gas with chlorine gas by thereaction represented below. A high-pressure bomb calorimeter is used for this experiment. A 500.-mLhigh-pressure cell is filled with an equimolar mixture of H,(g) and CL,(g) to a total pressure of10.00 atm and 293.50 K.H,(g) + CL(g) → 2 HCI(g)(a) If the reaction goes to completion, how many moles of HClI(g) can be produced?(b) The high-pressure sealed cell was placed in the bomb calorimeter and the mixture was ignitedwith an internal spark. The temperature of the calorimeter rose from 293.50 K to 298.83 K.If the previously-measured heat capacity of the whole calorimeter was C 3.60 kJ/K, calculatethe heat transferred to the calorimeter by the reaction.(c) Calculate the experimental enthalpy of reaction in kJ/moln

Volume of the gas = 500mL or 0.500L Pressure = 10atm Temperature = 293.50K Using ideal gas law, PV…

A student wishes to determine the enthalpy of the reaction of hydrogen gas with chlorine gas by the reaction represented below. A high-pressure bomb calorimeter is used for this experiment. A 500.-mL high-pressure cell is filled with an equimolar mixture of H,(g) and CL(g) to a total pressure of 10.00 atm and 293.50 K. H,(g) + CL,(g) → 2 HCI(g) a) If the reaction goes to completion, how many moles of HCI(g) can be produced? b) The high-pressure sealed cell was placed in the bomb calorimeter and the mixture was ignited with an internal spark. The temperature of the calorimeter rose from 293.50 K to 298.83 K. If the previously-measured heat capacity of the whole calorimeter was C 3.60 kJ/K, calculate the heat transferred to the calorimeter by the reaction. =) Calculate the experimental enthalpy of reaction in kJ/moln

A student wishes to determine the enthalpy of the reaction of hydrogen gas with chlorine gas by the reaction represented below. A high-pressure bomb calorimeter is used for this experiment. A 500.-mL high-pressure cell is filled with an equimolar mixture of H,(g) and CL(g) to a total pressure of 10.00 atm and 293.50 K. H,(g) + CL,(g) → 2 HCI(g) a) If the reaction goes to completion, how many moles of HCI(g) can be produced? b) The high-pressure sealed cell was placed in the bomb calorimeter and the mixture was ignited with an internal spark. The temperature of the calorimeter rose from 293.50 K to 298.83 K. If the previously-measured heat capacity of the whole calorimeter was C 3.60 kJ/K, calculate the heat transferred to the calorimeter by the reaction. =) Calculate the experimental enthalpy of reaction in kJ/moln

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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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

THERMOCHEMISTRY
237
23
3. A student wishes to determine the enthalpy of the reaction of hydrogen gas with chlorine gas by the
reaction represented below. A high-pressure bomb calorimeter is used for this experiment. A 500.-mL
high-pressure cell is filled with an equimolar mixture of H,(g) and CL,(g) to a total pressure of
10.00 atm and 293.50 K.
H,(g) + CL(g) → 2 HCI(g)
(a) If the reaction goes to completion, how many moles of HClI(g) can be produced?
(b) The high-pressure sealed cell was placed in the bomb calorimeter and the mixture was ignited
with an internal spark. The temperature of the calorimeter rose from 293.50 K to 298.83 K.
If the previously-measured heat capacity of the whole calorimeter was C 3.60 kJ/K, calculate
the heat transferred to the calorimeter by the reaction.
(c) Calculate the experimental enthalpy of reaction in kJ/moln

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