1 mol propane (C3H8) and stoichiometric amount of oxygen (O2) needed to combust propane was preheated to 400 K. After combustion, the products released are at 1500 K. The combustion products are H2O(l) and CO2(g). With 100% conversion was achieved, estimate the total heat released. Calculate the heat requirement for a reactor in combusting 1 mol of methane, CH4, with 25% excess air until the products reach a temperature of 1000 K. The reactants entered the reactor at 298.15 K and 100% conversion of methane is achieved. Assume air is approximately 21% O2 and 79% N2 and products are H2O(l) and CO2(g). Hint for both #1 and #2 – Combustion products at 298 K is CO2(g) and H2O(l). If the exiting temperature is above 373.15 K, H2O will leave as H2O(g). Therefore, you should account for the phase change of H2O(l) to H2O(g).

1 mol propane (C3H8) and stoichiometric amount of oxygen (O2) needed to combust propane was preheated to 400 K. After combustion, the products released are at 1500 K. The combustion products are H2O(l) and CO2(g). With 100% conversion was achieved, estimate the total heat released. Calculate the heat requirement for a reactor in combusting 1 mol of methane, CH4, with 25% excess air until the products reach a temperature of 1000 K. The reactants entered the reactor at 298.15 K and 100% conversion of methane is achieved. Assume air is approximately 21% O2 and 79% N2 and products are H2O(l) and CO2(g). Hint for both #1 and #2 – Combustion products at 298 K is CO2(g) and H2O(l). If the exiting temperature is above 373.15 K, H2O will leave as H2O(g). Therefore, you should account for the phase change of H2O(l) to H2O(g).

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.86PAE: The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a...

See similar textbooks

Similar questions

A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns then into gaseaous products. the cylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. the cylinder is also submerged in a large insulated water bath. From previous experiments, this chemical reaction is known to release 173.kJ of energy. the temperature of the water bath is monitored, and it is determined from this data that 37.2kJ of heat flows out of the system during the reaction. Is the reaction exothermic or endothermic? Does the temperature of the water bath go up or down? Does the piston move in or out? Does the gas mixture do work, or is work done on it? How much work is done on (or by) the gas mixture? Round your answer to 3 significant digits.
Methane (CH4) burns completely with 100% excess air in a steady-flow combustion process. Those entering and leaving the combustion process are at 25 C temperature and 1 atmosphere pressure, and the water between the end products of combustion is in the liquid phase. Calculate the heat transfer during the combustion process.
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 68.5 mL water (where X is a hypothetical metal): X + 2 HCI ---> XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 33.3 °C. If 0.00629 mol of "X" was consumed during the reaction, what is ?rH of this reaction in kJ mol^-1with respect to "X"? The specific heat of water is 4.184 J g-¹ °C-¹
Many barbeque grills use propane gas, C3H8(g) as a fuel source. Using standard enthalpies of formation, calculate the quantity of heat produced, in kJ, when 25 liters of liquid propane is completely combusted in air. (The density of liquid propane is 582 kg/m3.) Note: The propane is in the condensed liquid state in the tank but changes to the gas phase as it is released. Calculate the change in enthalpy for the reaction assuming all reactants and products are in the gas phase.
The n-butane is converted into isobutane in an isomerization reactor, which operates isothermally at 149°C. Suppose that the reactor is fed with a mixture containing 93% mole of n-butane, 5% isobutane and 2% HCl at 149°C and that a 40% conversion of n-butane is achieved. How much heat in KJ/m3 (STP) of the feed, should be supplied or extracted from the reactor?
The production of cement results in significant GHG emissions. The emissions are caused by the decomposition of calcium carbonate (limestone) to calcium oxide (lime) and carbon dioxide. This process known as calcination, is carried out in kilns. Therefore, additional GHGs are emitted as a result of heating the kilns. A large cement manufacturer uses a mix of coal, natural gas, and biomass in its boiler. This mix produces the following amounts of GHGs per Million BTUs of energy: • 250 lbs CO2/MMBtu • 5 lbs CH4/MMBtu • 0.36 lbs N2O/MMBtu Process carbon emissions from the calcination process produce 925 lbs of carbon dioxide per metric ton of cement. In addition, the plant uses 1.7 Million BTUs of energy per metric ton of cement. If the plant produces 180,000 metric tons of cement annually, how many metric tons of CO2e does it emit?
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 37.5C. During the reaction 92.8kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. Heat capacity of water is 4.18J.g-1.K-1. Round your answer to 3
A block of iron weighing 3.60 kg at a temperature of 807.0 °C was inserted into a container containing 1.00 liter of water at a temperature of 30.0 °C isolated from the environment. The cooling process of iron happens in two phases, the first phase the water is heated to the boiling point and in the second stage the water evaporates. This phase continues until the temperature of the iron is equal to the temperature of the water. The final temperature of the water and the iron is 100.0 °C. How many liters of liquid water will remain at the end of the process? (The specific heat of solid iron is 0.450 J g ̄1 K ̄1 and the heat of vaporization for water is 2259.23 J/g.)
A mixture of gaseous reactants is put in to a cylinder, where a chemical reaction turns them in to gaseous products. The cylinder has a piston that moves in or out as necessary to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a large insulated water bath. From previous experiments, this chemical reaction is known to release 211. kJ of energy. The temperature of the water bath is monitored, and it is determined from this data that 360. kJ of heat flows out of the system during the reaction. A)does The gas mixture do work, Or is work done on it? B)how much work is done on (or by) the gas mixture?
A mixture of gaseous reactants is put in to a cylinder, where a chemical reaction turns them in to gaseous products. The cylinder has a piston that moves in or out as necessary to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a large insulated water bath. From previous experiments, this chemical reaction is known to release 211. kJ of energy. The temperature of the water bath is monitored, and it is determined from this data that 360. kJ of heat flows out of the system during the reaction. A) is the reaction exothermic or endothermic? B) Does the temperature of the water go up or down? C) does the piston move in, out, or neither? D)does The gas mixture do work, Or is work done on it? E)how much work is done on (or by) the gas mixture?
A mixture of gaseous reactants is put in to a cylinder, where a chemical reaction turns them in to gaseous products. The cylinder has a piston that moves in or out as necessary to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a large insulated water bath. From previous experiments, this chemical reaction is known to release 211. kJ of energy. The temperature of the water bath is monitored, and it is determined from this data that 360. kJ of heat flows out of the system during the reaction. A) is the reaction exothermic or endothermic? B) Does the temperature of the water go up or down? C) does the piston move in, out, or neither?
You are camping and need to cook all your food using your camp stove which runs off of propane.If you wanted to warm up your giant mug (67.628 fluid ounces) of morning coffee from 10°C to 80°C,what mass of propane would you have to use?The ΔHcomb for propane is -2219.2 kJ/mol, the density of coffee is 1.0002 g/mL, and the specific heatcapacity of coffee is equal to that of water.1 fluid ounce = 0.0295735 L