There are 2 correct answers I suppose, II and III.
Gas pressure is increased if the molecules inside the container hit the inner wall of the container faster (more frequently), or harder. These are 2 ways of how the gas pressure of some gas is increased. We can figure out if the options will increase the gas pressure.
For I, removing part of the gas, this will remove part of the gas molecules. In result, fewer molecules will hit the wall because some are removed, like the number density is reduced. This does not increase the gas pressure, but instead decreasing it. So, option I is not correct.
For II, if the container size is decreased, the gas molecules have a shorter distance to travel before they hit the inner wall of the container, so, they hit the wall faster and more frequently. This can help increase the gas pressure, so option II is correct.
For III, if the temperature of the molecules is increased, the molecules will have a higher kinetic energy. They tend to move faster and of course eventually, they hit the inner wall of the container more frequently. In addition, if they have a higher kinetic energy, they'll even hit the inner wall harder, which can increase the gas pressure too. Therefore, option III is correct too.
The reaction between ammonium sulfate and calcium hydroxide is given below. (NH₄)₂SO₄ + Ca(OH)₂ --> 2NH₃ + CaSO₄ + 2H₂O From the balance equation, we can conclude that every 74 g of calcium sulfate reacted with enough amount of ammonium sulfate will yield 34 grams of ammonia. From the given amount, (20 g calcium sulfate) x (34 grams ammonia / 74 g calcium sulfate) = <em>9.19 g ammonia</em>
I would say, what helps me is really paying attention in class and asking questions, also making sure you study for upcoming test's and quizzes and completely assingments on time
