Oxy-acetylene torches can be used to cut or weld metal. Oxygen and acetylene are fed from separate compressed gas cylinders through pressure regulators to the torch where they are mixed and combusted. To estimate the amount of metal that can be cut or welded per unit volume of gas, the composition of the gases produced by combustion and heat produced by the combustion reaction must be determined. For this problem: a. Define a closed system that can be used to calculate the heat produced o. Define an open system that can be used to calculate the heat produced c. List at least two intensive variables that are important in calculation d. List at least two extensive variables that are important in the calculation

Oxy-acetylene torches can be used to cut or weld metal. Oxygen and acetylene are fed from separate compressed gas cylinders through pressure regulators to the torch where they are mixed and combusted. To estimate the amount of metal that can be cut or welded per unit volume of gas, the composition of the gases produced by combustion and heat produced by the combustion reaction must be determined. For this problem: a. Define a closed system that can be used to calculate the heat produced o. Define an open system that can be used to calculate the heat produced c. List at least two intensive variables that are important in calculation d. List at least two extensive variables that are important in the calculation

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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Please provide these answers 25. For an isochoric process, the thermal effect is equal to: changes in Gibbs free energy. changes in entropy of the system. enthalpy change of the process zero changes in internal energy. 26. System state functions depend on: the ability of the system to return to its initial state values of the chemical equilibrium constant exchange of matter and energy with the environment initial and final state of the system way of complying with the process 27. Heat and work depend on: exchange of matter and energy with the environment initial and final state of the system the ability of the system to return to its initial state values of the chemical equilibrium constant way of complying with the process
Suppose that 2.41 grams of X (MW 36.24) are dissolved in 595 mL of water, and the water temperature changes from 22.84°C to 20.45°C. Assume that the mass of X is negligible compared to the mass of the water. Assume the specific heat of water is 4.2 J/(g.°C) and the density of water is 1.0 g/mL. Calculate the enthalpy of dissolution of X in kJ/mol. Report your answer to three decimal places.
An 84 g sample of ethylene or ethene gas is reacted with 125 g of HCl gas in a system at At a constant volume, the heat generated can be used to raise the temperature of 1000 g of water from 25°C to 72°C. If it is known that the specific heat of water is 4.184 J.g-1.°C-1 , so : a. Write the equation for the reaction for ethylene. b. Calculate the change in energy (delta E) per mole of ethylene gas! c. If 70 g of ethylene gas reacts at atmospheric pressure and there is a change in volume from 100 liters to 65 liters, then what is the enthalpy change for the reaction? (1 L.atm = 101 J)
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Can you help me out with this one please. Thank you.
The results of your Solubility of a Salt experiment led to the following linear regression equation: ln(s)= -4197(1/T)+ 17.96 What is the heat of solution, ΔH, in kJ/mol? a. 25 b. 35 c. 45 d. 55
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Refer to the attached photo. Thank you!
A student dissolves 10.3g of ammonium nitrate NH4NO3 in 300.g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0°C to 19.3°C over the course of 3.1 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3s -> NH+4aq + NO−3aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔHrxn per mole of NH4NO3.
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