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m_a_m_a [10]
3 years ago
9

When the fuel mixture contained in a 1.49 l tank, stored at 750 mmhg and 298 k, undergoes complete combustion, how much heat is

emitted? (assume that the water produced by the combustion is in the gaseous state.)?
Chemistry
1 answer:
Ket [755]3 years ago
4 0
Get to know first how many moles in the gas:n = pV/RT= (1.013*10^5*750/760) Pa *1.49*10^-3 m^3/(8.314 J/(molK)*298) n = 0.0601 moles. 
The combustion energies  are  889 kJ/mol (methane) and 2 220 kJ (propane) x = moles methane, y = moles propane 
x*889 + y*2220 = 778 x + y = 0.0601----------- x = 0.267784 moles = 0.267784*100/0.0601 = 44.6 % y = 0.243216 moles = 0.243216*100/0.0601 = 55.4 %
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Explanation :

Endothermic reaction : When the system absorb heat from the surrounding then the surrounding become cool.

Exothermic reaction : when the system releases heat into the surrounding then the surrounding become hot.

According to the question,

when we mixed chemical A and chemical B together in a test tube to form chemical C, the mixture become cool. This means that the system is absorbing heat from the surrounding and thus the reaction is called a endothermic reaction.

And when we added chemical D in chemical C, the new mixture becomes hot and explodes. This means that the system is releasing heat into the surrounding and thus the reaction is called as exothermic reaction.


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The amount of electric charge that can build up across a unit length, unit area, or unit volume of a conductor is known as charge density. In other words, it shows the amount of charge that is held in a certain field. It determines how the charge is distributed and can be either positive or negative.

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