There was a drop in kinetic energy, so the vapor pressure inside of the can became extremely low. The drop in pressure meant that the molecules hit the sides of the can with less force and hit the sides less frequently. The pressure inside of the can was then much lower than the atmospheric pressure outside. The molecules outside crushed the can because when they hit the outside of the can, they hit it more frequently and with more force compared to the molecules inside of the
Collisions increase or become more violent between molecules at higher temperatures or decrease as the temperature is lowered. Some factors that influence the speed of a chemical reaction are: (1) surface area of starting reactants; (2) concentration of reactants; (3) temperatures. The particle theory states that a solute dissolved takes place at the surface of the solvent and the larger the surface area of the particle the longer it will take to dissolve. The smaller the area the faster it will
Since the solution became a dark red, the concentration of FeNCS2+ had increased. The darker solution means that the products are more favored at equilibrium which is called product favored and a lighter solution means that the reactants are more favored at equilibrium which is called reactant favored. When the group added more Fe(NO3)3 or NH4NCS to the second experiment, the system reacted by
This column – of a large surface area with glass or ceramic – provides ample contact between the vapor and liquid phases. A temperature gradient is formed because the head of the system is now further from the flask. Factors that affect the temperature gradient include the rate of heating and vapor removal from the system’s stillhead. Upon heating, the vapor of compound A rises, reaching a distance at which it no longer has enough energy to maintain its gaseous form; at this point, the molecules re-enter the liquid state. This process of rising up, condensation, and revaporization eventually results in vapor comprising 100% of substance A.
The melting point for lauric acid in this experiment was 50℃. Explain what is happening during each section of the graph for both cooling and heating in terms of particle motion and energy. When heat is added to a substance the particles in the substance vibrate faster and when vibrate faster the space between the particles increases. The hotter it gets the more the object expands and takes up more space. When a substance is cooled the particles vibrate less causing them to constrict and take up less space.
The difference between the rates of the reaction’s when 1 mole was inserted, and when the 3 mole was inserted is 118.49 seconds. This is the data the proves that my hypothesis is correct, this is because as the amount of mole increase, the amount of energry included in the reaction is more. for example, take the 1 mole of HCL, the 2 mole of HCL, and the 3 moles of HCL. The 1st mole of HCL has more particles than the 2nd mole of HCL, and thus when the 1st mole reacts with HCL, the rate of the reaction will be more because there will be more less energy in the reaction of HCL and Mg, compared to the 2nd mole of HCL and it reaction with Mg, (the 2 moles of HCL has more energy than the 1 mole), so hence, there will be more energy in the reaction . Both mole of HCL(the 2 moles of HCL and the 1 mole of HCL) have less energy , and thus when the 3 moles of HCL reacts with Mg, there is even more energy between the Mg and the HCL particles, so hence the rate of the reaction will be faster.
As shown in Figure 1, the pansey under humid conditions had the smallest negative percent change in mass through transpiration. As said before, the background states that water potential is the measure of the potential energy of water that water flows from areas of high water potential to low water potential. It also states that humidity decreases transpiration by increasing the water potential of the air, therefore causing less water to be evaporated into the atmosphere. From this, it can be determined that since the humid environment provided a moist atmosphere, the water potential of the air increased causing there to be little transpiration from the leaves due to the gap between the two water potentials being so small. This supports the hypothesis which stated that when placed in a humid environment, the pansy will experience a negative percent change in mass that is significantly less than that of the
This is evident from the following figure. Figure 24 SEM images of (a) Sample with Tsat=200C, Tf=1100C and RD=84.1; (b) Sample with Tsat=00C, Tf=900C and RD=84.1. (Courtesy to ) Effect of foaming temperature on cell nucleation density and average cell size Variation in nucleation densities with temperature can be observed in the following figure Figure 25 Cell nucleation density as a function of foaming temperature for samples foamed at different saturation temperature. (Courtesy to ) The nucleation density increases with a decrease in foaming temperature. Cell nucleation density as high as 1014 cells/cm3 were obtained for saturation temperature of -100C for which CO2 concentration was 14.7% whereas for a saturation temperature of 600C the nucleation density was 109 cells/cm3 where CO2 concentration was 5%.
Applying this statement to the experimental setup, the average kinetic energy of the molecules of warm water is therefore much higher than that of the cold water. So, the molecules of warm water are actually able to occupy more space because of their rapid velocities and high kinetic energies. Because the constituent particles of the warm water occupy more space, the substance is therefore low in density. Now, there are not many differences between the properties of warm water and cold water in the experiment — including mass. Nonetheless, it is the disparity in temperature and density of the water that accounts for the results of the experiment.