hello
You can use the ideal gas law, PV = nRT, to solve for the number of moles, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Rearrange the formula to solve for n, n = (PV) / (RT). Convert the temperature from Celsius to Kelvin (27°C + 273 = 300 K), and plug in the values to find the number of moles of the gas in the container.
The term gas is limited to those substances that exist in the gaseous state at room temperature and pressure. This means they have low density, take the shape of their container, and have molecules that are far apart. Gases can be compressed and expand to fill their container.
Gaseous iron is highly reactive and can easily react with the glass container, causing it to break or degrade. Additionally, the high temperatures required to keep iron in a gaseous state would likely cause the glass to shatter.
The production of ammonia from gaseous hydrogen and gaseous nitrogen will increase at a higher temperature. This is because the reaction is endothermic, meaning it requires heat to proceed. Higher temperatures provide the necessary energy for the reaction to occur more rapidly.
The reaction between chlorine gas and fluorine gas yields a gaseous product with formula ClF3. This is because the ratio of volumes (1:3) corresponds to the molar ratio in the balanced chemical reaction: 2Cl2 + 3F2 → 2ClF3.
Decreasing the temperature and increasing the pressure will decrease the total amount of gaseous solute able to be dissolved in a liter of liquid water. Conversely, increasing the temperature and decreasing the pressure will increase the amount of gaseous solute that can be dissolved.
Decreasing the temperature of the system would NOT cause an increase in pressure. According to the ideal gas law, pressure and temperature are directly proportional when other variables are constant. Therefore, decreasing the temperature would result in a decrease in pressure.
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
Opening a can of soda is not a chemical reaction because no new substances are formed. It is a physical change where no chemical bonds are broken or created. The release of gas when the can is opened is due to the pressure change, not a chemical reaction.
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).
Gas exerts pressure on the walls of its container through the continuous collisions of gas molecules with the container walls. The higher the frequency and force of these collisions, the greater the pressure exerted by the gas. This interaction is described by the kinetic theory of gases.
The concentration of reactants is changed.If the reaction occurs in the gas phase
No, the addition of a noble gas does not affect the partial pressures of the other gases in a gaseous equilibrium system. Noble gases are considered inert and do not participate in the equilibrium reactions. They simply occupy space in the container without interacting with the other gases present.
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 :)