ΔH0 (kJ/mol)
C2H2 (g) = 226.7
C6H6 (g) = 82.9
S0(J/mol*K)
C2H2 (g) = 200.8
C6H6 (g) = 269.2
Cp
C2H2 (g) Cp = 30.7 + 5.28*10-2 T + 1.63*10-5 T2 (J/mol*K)
C6H6 (g) Cp = -1.7 + 3.25 *10-2 T - 11.06*10-5 T2 (J/mol*K)
Compute ΔH(Temperature Final)reaction and ΔS(Temperature Final)reaction
Initial Temperature = 298.15K
Final Temperature = 330K
ΔH0 (kJ/mol) C2H2 (g) = 226.7 C6H6 (g) = 82.9 S0(J/mol*K) C2H2 (g) = 200.8 C6H6...
Given the following table of thermodynamic data, substance S° C2H2 (g) 200.8 J/mol −K C2H4 (g) 219.4 C2H6 (g) 229.5 H2 (g) 130.58 determine the D S° (in J/mol −K) for the reaction: C2H2 (g) + H2 (g) ® C2H4 (g) −111.98 −101.88 −232.46 +111.98 +101.88
AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 0 0 130.7 Hydrogen H2 (g) H (g) H' (g) H+ (aq) 218.0 203.2 114.7 1536.2 0 -230.0 -157.0 -11.0 -285.8 -237.1 69.9 OH(aq) H20 (1) H20 (g) H2O2 (1) -241.8 -228.6 188.8 -187.8 -120.4 109.6 Iodine AH.(kJ/mol). | AGO. (k.I/mol) go (I/mol K | -53.0 -13.0 242.0 -277.7 -174.8 160.7 282.7 -235.1 -484.0 160.0 C2H40 (g, ethylene oxide) CH3CH2OH (1) CH3CH2OH (g) CH3COOH (1) C2H6 (g) C3H6 (g) CzH; (g) CH2=CHCN (1)...
A) 2PbS(s)+3O2(g)→2PbO(s)+2SO2(g), ΔH∘=−844 kJ, ΔS∘=−165 J/K Express the Gibbs free energy in kilojoules to three significant digits. B) 2POCl3(g)→2PCl3(g)+O2(g), ΔH∘=572 kJ, ΔS∘=179 J/K Express the Gibbs free energy in kilojoules to three significant digits. C) At what temperature (if any) would the decomposition of POCl3 become spontaneous? Express the temperature in kelvins to three significant digits. If there is no answer, enter none.
1.) The specific heat of a certain type of metal is 0.128 J/(g⋅∘C). What is the final temperature if 305J of heat is added to 41.7 g of this metal, initially at 20.0 ∘C? 2.) When 1723 J of heat energy is added to 42.3 g of hexane, C6H14, the temperature increases by 18.0 ∘C. Calculate the molar heat capacity of C6H14 3.) Liquid sodium is being considered as an engine coolant. How many grams of liquid sodium (minimum) are...
1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol Which of the following is true? ΔG = -44.8 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will be spontaneous ΔG = -44.8 kJ/mol and the process will be spontaneous ΔG = -19.1 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will not be spontaneous 2. Consider a...
FR 5. (15 points) Two blocks one of aluminum (Al MM= 26.98g/mol , Cp,m=24.35 J/mol K), the other of silver (Ag MM= 107.9 g/mol , Cp,m 25.351 J/mol K) of mass (100 g) are at two different temperatures (TAI=300K and Tag=500K). Calculate the change in entropy for the system once the final temperature is achieved.
For the reaction shown below, ΔH° = -61.9 kJ mol-1 and ΔS° = -76.7 J K-1 mol-1. Si (s) + 2 H2 (g) ⇌ SiH4 (g) Choose one of the following: TOWARD PRODUCT, TOWARD REACTANT, NO CHANGE to describe what will happen in each of the situations described below (5 pts each) a. If some Si(s) is added to the system the equilibrium will shift b. If some H2 (g) is removed from the system, the equilibrium will shift c. If the...
the following equations is the balanced combustion reactions for c6h6 2C6H6(l)+15O2---->12CO2(G)+6H20(l)+6542 k j if 7.700 g of C6H6is burned and the heat produced from the burning is added to 5691 g of water at 21 c what is the final temperature of the water?
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 270.0 K is Assume that AH° and AS are independent of temperature. Submit Answer Try Another Version 3 item attempts remaining elefchces to access important values if needed for this question, Consider the reaction 2CO2(g) + 5H2(g)CH2(g) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if...
Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) N2 (g) 0 0 191.6 472.7 455.6 153.3 N(g) NH3 (g) -46.1 -16.5 192.5 NH3 (aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO (g) 90.3 86.6 210.8 NOCI (g) 51.7 66.1 261.8 NO2 (g) 33.2 51.3 240.1 N20 (g) 82.1 104.2 219.9 N204 (8) 9.2 97.9 304.3 Consider the reaction N2(9) + 202(9)—2NO2(g) Using the standard thermodynamic data in the tables linked above, calculate Grxn for this reaction at 298.15K...