If the reaction is not spontaneous under standard conditions at 298K, at what temperature (if any) would the reaction become spontaneous? a) 2 PbS (s) + 3 O2 (g) → 2 PbO (s) + 2SO2 (g) ; ΔH° = -844 kJ; ΔS°= -165 J/K b) 2 POCl3 (g) → 2 PCl3 (g) + O2 (g) ; ΔH° = 572 kJ; ΔS°= 179 J/K 5. Consider the reaction H2 (g) + F2 (g) → 2 HF (g). a) Using data in your Appendix B, calculate ΔG° at 25°C b) Calculate ΔG at 298K if the reaction mixture consists of 8.0 bar of H2, 4.5 bar of F2 and 0.36 bar of HF. 6.
1 / [CO2] C. [CaO][CO2] / [CaCO3] D. [CaCO3] / [CaO][CO2] _____ 13. The value of Kp for the reaction 2 NO2 (g) [pic] N2O4 (g) is 1.52 at 319 K. What is the value of Kp at this temperature for the reaction N2O4 (g) [pic] 2 NO2 (g) ? A. -1.52 B. 1.23 C. 5.74 X 10-4 D. 0.658 _____ 14.
a) for a we first need to find a balanced equation for when the hydrocarbons combust to form CO2 and H20. Then we plug in the deltaHf values and plug these into the equation. a) C4H6 + 11/2O2 ==> 4CO2 + 3H2O Delta Hrxn = [4DeltaHf(CO2)+3DeltaHf(H2O)] - [DeltaHf(C4H6) + 11/2DeltaHf(O2)] = [4(-393.5kJ) + 3(-285.83kJ)] - [111.9kJ + 11/2(0kJ)] = -2543.39kJ C4H8 + 6O2 ==> 4CO2 + 4H2O Delta H rxn = [4DeltaHf(CO2) + 4DeltaHf(H2O)] - [DeltaHf(C4H8) + 6DeltaHf(O2)] = [4(-393.5kJ) + 4(-285.83kJ)] - [1.2kJ +6(0kJ)] = -2718.52kJ C4H10 +13/2O2 ==> 4CO2 +5H2O DeltaHrxn = [4DeltaHf(CO2) + 5DeltaHf(H2O)] - [DeltaHf(C4H10) + 13/2DeltaHf(O2)] = [4(-393.5kJ) + 5(-285.83kJ)] - [-124.7kJ +
3) Write equations to indicate what you consider to have happened in each case in which there was precipitate formed. Use ions to represent the species in the reacting solutions, but for those products that were precipitates write a formula for the compound. Place (aq) after those species in solution and (s) after the precipitates. Be sure to write the equations so that both atoms and charge are conserved. For example: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) ( AgCl(s) + Na+(aq) + NO3-(aq) 4) Rewrite the equations, leaving out the ions not involved in the reaction (spectators).
Abstract The focus of this experiment was to analyze the kinetics of a nucleophilic substitution. A mixture of 0.3622-M 1-bromopropane and 0.3622-M potassium hydroxide in an 90:10 ethanol/water solvent provided the reactants for a SN2 reaction to occur in a temperature controlled bath at 50.0˚C. The disappearing reactant was found by titrating timed aliquots during the reaction and then measuring the concentration of hydroxide. The k-value was found to be 0.0202 M-1Min-1. Using the linear form of the Arrhenius equation the activation energy was calculated to be 19.9 kcal/mol.
When an electrolyte or non electrolyte is introduced the effectiveness of the Boiling point changes. III. Data Table A. Boiling points of the solution Solution- NaCl + H2O Temperature measured for 30 Seconds Trial 1 101.3 ̊ C Trial 2 101.7 ̊C Trial 3 102.5 ̊̊C Average of trials 101.8 ̊C IV. Computations A. Calculations in Lab Writeup 1.
Predict the number of valence electrons for a chlorine atom. a. 1 b. 5 c. 7 d. 17 e. 35 Ionization Energy 59. Which of the following is a general trend for the ionization energy of elements in the periodic table?
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.
(b) The energy for ATP synthesis is furnished by light-induced electron transfer in the chloroplasts. What is the minimum voltage drop necessary (during transfer of a pair of electrons) to synthesize ATP under these conditions? (You may need to refer to Eqn 13–7, p. 515.) Answer (a) G G RT ln [ATP] [ADP][Pi] (2.48 kJ/mol) ln 1.2 10 4 10 6) (7.0
Title: SOME AQUEOUS SOLUTION CHEMISTRY OF COPPER(II)ION Aims: 1. To make the synthesis of Copper(II) Sulfate Pentahydrate and determine the theoretical yield as well as the percent yield of CuSO4.5H2O 2. To observe a series of reactions with copper (II) ions using different reagents. Results & Questions: A. Synthesis of Copper(II) Sulfate Pentahydrate. 1.