Gaseous Reaction Lab

Think about the gas laws we are studying. Boyle’s law tells us that pressure and volume are inversely proportional. Charles’ law states that volume and temperature are directly proportional. We also know that pressure and temperature are directly proportional. Discuss at least one instance in your personal experience where you have seen one or more of these laws in action.

What happens to the equilibrium price and quantity after these changes are put into effect? Do they go up, down or stay the same?P:_____down_____________Q:_____down__________________

is initially in both short and long run equilibrium [Hint: Your diagrams for each part should look

The purpose of this experiment was to determine the effect of a change on a system at an equilibrium. I will learn how temperature and pressure affects a chemical reaction. During this experiment, I will observe the physicals changes when the solutions are mixed and determine the shift of the equilibrium. I think the only reaction I will have will be color change, when the different solutions are added together.

At the new equilibrium point E2, the equilibrium quantity shifts inward to 4,000,000 barrels. There is a deadweight loss of $1 trillion which the market cannot account for as shown in the triangle depicted on the graph.

All equilibrium reactions have a corresponding

Equilibrium is a state in a reaction in which both the reactants and the products are present in concentrations that are both constant, and will not change over time. This state results when the forward reaction is proceeding at the same rate as the reverse reaction. An example of this can be seen in the dissolution of Sodium Chloride in water. If the equilibrium equation NaCl(s) NaCl (aq) is used, we can see that the compound in the solid form is re-crystalizing at the same rate as the aqueous form is dissolving. There are 3 main disturbances that can alter equilibrium, a change in concentration of reactants or products, a change in temperature or a change in pressure. According to Le Chatelier’s principle, if any of these three is disturbed, the system compensates by shifting the equilibrium to either the left or the right. This can be seen in the equilibrium reactions associated with sea water. In the dissolution process of CO2 discussed before, not all of the CO2 molecules remain dissolved. A small amount react with the water to form carbonic acid (H2CO3), which can be seen in the equation CO2 (aq) + H2O H2CO3 (aq). As carbonic acid is a weak acid, it can dissociate to bicarbonate or carbonate. These two equations respectfully are H2CO3 (aq H+ (aq) + HCO3- (aq),

Equilibrium is when a reaction ratio becomes unbalanced. In the reaction, it does not affect the outcome if the reactants like chromate & hydrogen chloride are not equal to the product water, dichromate, and chloride ion. As long as the reaction maintains the same ratio it won't matter if it's a forward or reverse reaction.

Pressure caused by gases and gases being placed under pressure is used in our everyday life. Without the use of gases we would be unable to fly in airplanes, play basketball or even have carbonated drinks. “Gases exert pressure on any surface with which they come in contact, because gas molecules are constantly in motion. We humans have adapted so well psychologically to the pressure of the air around us that we are usually unaware of it” (Chang 155). The equation often used to measure the pressure of gases is the ideal gas equation P=nRT/V. Where P is the pressure of the gas in atm, n is the number of moles of gas, R is the proportionality constant (0.0821 L*atm) T is the temperature in Kelvin of the gas, and V is the volume the gas occupies (Chang 160).

When the temperature of the gas was lowered, and the volume was constant the pressure inside decreased. This was caused because more kinetic energy results in higher pressure levels, so if the kinetic

Once a reaction has reached its chemical equilibrium it consists of a point where the rates of the forward and reverse direction of a reaction equal each other. Since at this point there is no movement that needs to take place the chemical process can be considered to be stabilized. When a reaction has reached equilibrium, the reactants become products and the products decompose into the reactants at the same rate (Gas-Phase, 2014). In other words, the forward reaction must occur at the same rate as the reverse reaction. This all can be associated with Le Chatelier’s principle, which indicates that if the equilibrium is disturbed by any condition it will modify itself towards the direction of the change until it is fully balanced. (Gas-Phase,

The position of equilibrium for the two competing directions is affected by the reaction conditions. The removal of a reactant would give about the reverse of the reaction. Thus, the removal of water or the reactant norbornene itself would shift equilibrium in the direction as to form more norbornene and water, and thus favoring the dehydration of

. The author used the example of the reaction of sodium and chlorine to support the postulate of chemical reaction. That during chemical reactions the atoms are rearranged in the reacting substances, to give a new chemical combinations present in the substances formed by the reaction, in this case salt.

Changes in the equilibrium price and quantity depend on exactly how the curves shift (Berkeley University, n.d.).

On day 3 firm 2 will expect firm 1 to continue its previous output level so keeps it own output level unchanged. Yet firm 1 cuts its output, this being a lagged response to the entry of firm 2. Therefore day 3 output combination is on 1'd reaction curve but not on 2's reaction curve. Given the shapes of the reaction curve as the process continues it converges on the Cournot equilibrium which is a stable.