Gas Equilibriums: Examples of Reversible Reactions Essay examples

Table 1: Reaction ICE Table Fe3+(aq) Initial Concentration Change in Concentration Equilibrium Concentration [Fe3+]i –x [Fe ]i – x

Aim: The aim of the lab “Chemical Equilibrium” is to observe the effects of changes in concentrations of products and reactants on the position of the equilibrium of given chemical reactions.

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.

* From the scenario for Katrina’s Candies, examine the key factors affecting the demand for and the supply of a good in general and Katrina’s Candies specifically. Distinguish between a change in demand and a change in the quantity demanded (movement along the demand curve).

The pressure of a gas sample increases for a decrease in volume and decreases for an increase in volume.

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

25) Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s) A) Ni B) Ag C) Cl D) O E) This is not an oxidation-reduction reaction. 26) How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°C and 755 mm Hg pressure according to the chemical equation shown below? BaH2(s) + 2 H2O(l) → Ba(OH)2(aq) + 2 H2(g) A) 1.60 L B) 3.21 L C) 0.799 L D) 0.219 L 27) A gas mixture contains CO, Ar and H2. What is the total pressure of the mixture, if the mole fraction of H2 is 0.35 and the pressure of H2 is 0.58 atm? A) 2.1 atm B) 0.60 atm C) 0.49 atm D) 1.7 atm E) 0.20 atm

Both experiments were able to determine the yield of hydrogen gas by testing the effect of limiting reactants, balanced equations, stoichiometry, mole ratios and molar masses. Balanced equations are equations that have a balanced number of moles of each element on both sides of the equation. Molar mass is the sum of the atomic masses of all elements combined in a chemical substance. Mole rations can be determined using the coefficients of the reactants and products in the balanced equation. Mole ratios can be used to relate moles of product formed from a certain number of moles of a reactant. Stoichiometry is the method of using the relationship between two or more substances in a chemical reaction. The limiting reactant of a chemical reaction is the reactant that is used up first in the reaction and limits how much of the product can be formed. In experiment 2-1, a company wanted to know if magnesium or aluminum would be practical to use as an alternative to zinc to produce a given volume of hydrogen gas. In experiment 2-2, the company wants to know how to optimize the production of hydrogen gas and whether hydrochloric or sulfuric acids are reasonable alternatives for gas production. The The reactions performed in experiment 2-1

The law of thermodynamics in can predict the direction of chemical reactions and changes in substances

What is the effect on the equilibrium price and equilibrium quantity of orange juice if the price of apple juice decreases and the wage rate paid to orange grove workers increases?

The k value in run 2 is nearly double that of run 6. This is directly related to the ∆t found for each, with ∆t2 being half that of ∆t6. This is a result of the H2O being present in run 6 while (NH4)2SO4 being present in run 2.

formula Kw[Fex(C2O4)y]·zH2O. The variables x, y, and z were determined through the duration of the

In this experiment, a redox reaction occurred. An oxidation-reduction reaction (redox) is a type of chemical reaction that involves a transfer of electrons between two solutions. The chemical being oxidized is losing electrons and the chemical being reduced is gaining electrons. In this case KMnO4 is losing electrons and Oxalic Acid is gaining electrons. KMnO4 can titrate a or reduce Oxalic acid. Titration is the technique used to find the unknown concentration of one solution based on the concentration of a known solution. In equation 2, the molar relationship between the 2 is shown, it is 2 KMnO4 to 5 Oxalic Acid. The molar ratio relationship is useful because it shows how much of a certain product is needed to help a reaction occur and which chemical is limiting reagent. The experiment was started by preparing a titrating strength KMnO4 solution from stock to a less concentrated KMnO4. Equation one shows how this was done. The KMnO4 needed to be diluted, if it had not been diluted, then it would be way too hard to get an accurate reading of the Oxalic Acid used. Without being diluted the Oxalic Acid would be strong. The next step was to standardize the KMnO4 solution. It was calculated that 37.5 mL of Oxalic Acid could titrate 15 mL of KMnO4. To determine the exact molarity of a solution a standardization needs to happen. In this experiment the standardization found how much Oxalic acid was needed. Through the controlled variable, the fact that 37.5 Oxalic acid could be titrated by 15 mL of KMnO4, the percent of the

Evaluate each of the following changes in supply and/or demand. How will each affect equilibrium price and quantity in a competitive market? Will price and quantity rise, fall, or be unchanged? Based on shifts, will the answers be indeterminate?

Using appropriate diagrams, discuss how an increase or an improvement in the following non-price determinants of supply would change equilibrium prices and quantities.