- 92
- 0
What are all the given aspects of this?
I understand how the reaction happens, but what about it pushes the piston.
I understand how the reaction happens, but what about it pushes the piston.
Last edited:
An increase of pressure........ what about it pushes the piston.
Caused by the molecular expansion due to the exothermic reaction?It's the pressure.
A mole of an ideal gas occupies 22.4 liters at standard temperature and pressure. Gasoline combustion gasses are not ideal but you get the idea.Caused by the molecular expansion due to the exothermic reaction?
Where is the pressure coming from?
Actually, in my opinion there is the electrical force (or electro-magnetical force) which pushes the piston. The fact that in the explosion the atoms are generating smaller molecules and reorganize, make increase drastically the volume.What are all the given aspects of this?
I understand how the reaction happens, but what about it pushes the piston.
Besides the Temperature increase, there is a very high increase in the 'n' of the equation -number of moles-. The gasoline enters as liquid and changes into gas.If you need an equation, the ideal gas law should be a first crude approximation : PV = nRT. The temperature in the cylinder clearly increases as the fuel/air mixture burns, and whatever gas is present has to increase either P, V or both to satisfy the gas law. Since the cylinder is made of solid steel, the only way V is going to increase is by having the piston head move away, bringing along a crankshaft rotation.
The increase is very modest. you get something likeBesides the Temperature increase, there is a very high increase in the 'n' of the equation -number of moles-. The gasoline enters as liquid and changes into gas.