hello
the reaction would shift to favor the side with the most moles of gas. (apex).
5535kJ is the reaction that represents breaking all the bonds in gaseous benzene C6H6.
Vapour is not a chemical reaction; instead, it is a tangible substance in a gaseous state and has no necessary association with chemical reaction at all.
A liquid
ClF3
the container is made larger
the reaction would shift to favor the side with the most moles of gas
the reaction would shift to favor the side with the most moles of gas
Nope. The pressure keeps the Carbon Dioxide dissolved in the liquid, and when that pressure is relieved, the CO2 rapidly returns to its gaseous state. None of the molecules are reacting or changing, although the CO2 switches from aqueous to gaseous phase.
the reaction would shift to favor the side with the most moles of gas. (apex).
the reaction would shift to favor the side with the most moles of gas. (apex).
the reaction would shift to favor the side with the most moles of gas. (apex).
the reaction would shift to favor the side with the most moles of gas. (apex).
The gaseous molecules are in continuous random motion and during their motion continuously strike the walls of container and exert the force on walls,the force per unit area is the pressure of the gas.
The concentration of reactants is changed.If the reaction occurs in the gas phase
Yes. If the pressure is increased, even with a noble gas, the reaction equilibrium will shift to alleviate and lower that increased pressure (if there are more moles of gas on one side of the reaction than the other).
Particles in gases, like the gas inside the balloon, move around a lot, fill up their container and collide a lot, both with each other and the walls of the container (ie - the balloon). Pressure is just how many collisions there are. So high pressure is when the particles collide with the walls of the container loads, and low pressure is when they don't collide with it very much. So the gaseous particles collide with the inside of the balloon, creating pressure. Hope that helps :)