A spherical balloon initially contains 25m3 of helium gas at 20o C and 150 kPa. A valve is now opened and the helium is allowed
to escape slowly. The valve is closed when the pressure inside the balloon drops to the atmospheric pressure of 100 kPa. The elasticity of the balloon material is such that the pressure inside the balloon during the process varies with the volume according to the relation P= A + BV where P is the pressure in kPa, V is the total volume in m3 , the constant A has a value of -100 kPa (i.e. negative 100kPa), and the constant B has an unknown value. The temperature at which the helium exits the balloon is constant at 15o C throughout the whole process.
Disregarding any heat transfer, determine
(a) the final temperature of helium in the balloon after the valve has been closed, and
(b) the mass of helium that has escaped. Consider helium to be an ideal gas with constant specific heats [5.193kJ/(kg K) for Cp,o and 3.116kJ/(kg K) for Cv,o].
Disregarding any heat transfer, determine
(a) the final temperature of helium in the balloon after the valve has been closed, and
(b) the mass of helium that has escaped. Consider helium to be an ideal gas with constant specific heats [5.193kJ/(kg K) for Cp,o and 3.116kJ/(kg K) for Cv,o].
1 answer:
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Taking into account the reaction stoichiometry, 340.0 moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas
<h3>Reaction stoichiometry</h3>In first place, the balanced reaction is:
CO₂ + 4 H₄ → CH₄ + 2 H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- CO₂: 1 mole
- H₄: 4 moles
- CH₄: 1 mole
- H₂O: 2 moles
The following rule of three can be applied: if by reaction stoichiometry 1 mole of CO₂ form 4 moles of CH₄, 85.1 moles of CO₂ form how many moles of CH₄?
<u><em>moles of CH₄= 340.4 moles</em></u>
Then, 340.0 moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas
Learn more about the reaction stoichiometry:
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