a. decreasing the temperature b. changing the concentration of A c. changing the concentration of B d. changing the concentration of C e. letting the reaction go on for a long time 4. The gas phase reaction A + B C has a reaction rate which is experimentally observed to follow the relationship rate = k[A]2[B]. If the concentration of A is tripled and the concentration of B is doubled, the reaction rate would be increased by a factor of ____. a. 6 b.
2. Explain what relationship exists between the pressure and volume of a gas (assuming a constant temperature), based on your collected data. Answer: The relationship between Pressure and Volume is inversely proportional. As one decrease, the other increases. P1V1=P2V2 3.
Background: A reaction rate is the decrease in concentration of a reactant or the increase in concentration of a product with time. Thus, the units for the reaction rate are usually Molarity per second (M/s) – that is , the change in concentration (measured in molarity) divided by a time interval (seconds in this case) (Chemistry: The Central Science, P. 527). Rate is usually calculated by taking an average of the disappearance or appearance of a compound with respect to time. In this case it is calculated by the absorbance of the light. Reaction rate is affected by any catalysts present (which speed up the reaction usually with an intermediate step), temperature (increases the number of particles collisions), concentration (increases the number of collisions), and surface area (increases the space available for collisions).
If the reaction is first order, its graphical representation is seen as ln[A] (natural log of concentration) vs. time, and the slope of its like is also the negative rate constant. Finally, for a second order reaction the graph is shown as 1/[A] (inverse of concentration) vs. time, and the slope of its given line is the positive rate constant. By understanding the rate law and finding the value of the correct rate constant with respect to the order of the reaction, one can determine the half-life of the crystal violet. This is because the crystal violet undergoes a decay reaction with the sodium hydroxide. According to Beer's Law, the absorbance of crystal violet is proportional to its concentration.
Any increase in the rate of reaction will cause an increase in the pressure of the oxygen. The first line of the graph (top) represents the normal rate of the reaction in a water solution of hydrogen peroxide and catalase. The second line represents the rate of reaction when acid is added to the solution and the third line represents the rate of reaction when a base is added to the solution. 1. What variable is plotted on the x-axis?
Lesson 13.6 Changes of physical state: * necessary to draw a temperature-energy graph to see the change in temperature with a constant application of heat Heat of fusion - the amount of heat required to melt 1.00 g of substance. substance changing from a solid to a liquid. Heat of vaporization - the amount of heat required to vaporize 1.00 g of a substance. substance changing from a liquid to a gas. heats of vaporization and condensation are equal.
The balanced equations for this reaction shows that the molar ratio of magnesium reacted to hydrogen gas produced is 1:1. Therefore, by determining the mass of magnesium that reacts and the number of moles that this mass is equal to, you will also be able to determine the number of moles of hydrogen gas produced. The volume of hydrogen gas produced will be measured directly on the scale of a gas-measuring tube. The gas laws of Boyle and Charles will be used to correct this volume, measured under laboratory conditions, to the volume the sample of gas would occupy at STP. The collected data (number of moles and volumes at STP) will be used to calculate that molar volume of the hydrogen gas.
Calculate the value of Ke for this system. 2 H2S (g) === 2 H2 (g) + S2 (g) [1.1(10-4] 7. At a given temperature, the following system has an equilibrium constant, Ke, of 0.27. C(g) + B(g) === 2 E(g) The system was established by placing 8.00 moles of C and 5.0 moles of B in a 4.0 L vessel. Calculate the concentration of all substances at equilibrium.
Using the G° data in your Appendix B, calculate the change in Gibbs free energy for each of the following reactions. In each case, indicate whether the reaction is spontaneous under standard conditions. a) H2 (g) + Cl2 (g) → 2HCl (g) b) MgCl2 (s) + H2O (l) → MgO (s) + 2 HCl (g) c) 2 NH3 (g) → N2H4 (g) + H2 (g) d) 2 NOCl (g) → 2 NO (g) + Cl2 (g) 4. From the values given for ΔH° and ΔS°, calculate ΔG° at 25°C for each of the following reactions. If the reaction is not spontaneous under standard conditions at 298K, at what temperature (if any) would the reaction become spontaneous?
The ULTIMATE Chemistry Semester 2 Study Guide! Iron: Fe+2 is ferrous Fe+3 is ferric Copper: Cu+1 is cuprous Cu+2 is cupric Lead: Pb+2is plumbous Pb+4 is plumbic Tin: Sn+2 is stannous Sn+4 is stannic Periodic Table TRENDS * As you move right along the periodic table… decreasing atomic radius, increasing ionization energy, increasing electronegativity, increasing electron affinity, constant shielding * As you move down the periodic table… increasing atomic radius, decreasing ionization energy, decreasing electronegativity, increasing shielding WTF is that stuff? * Atomic radius is the distance between the nuclei of atoms when they are involved in a chemical bond. As you increase the number of protons in the nucleus