Given:
Hof(A) = -78.0 KJ/mol
Hof(B) = -82.0 KJ/mol
Hof(C) = -80.0 KJ/mol
Hof(D) = -75.0 KJ/mol
Balanced chemical equation is:
2 A + B ---> 2 C + 3 D
ΔHo rxn = 2*Hof(C) + 3*Hof(D) - 2*Hof( A) - 1*Hof(B)
ΔHo rxn = 2*(-80.0) + 3*(-75.0) - 2*(-78.0) - 1*(-82.0)
ΔHo rxn = -147 KJ
Given:
Sof(A) = 194.0 J/mol.K
Sof(B) = 183.0 J/mol.K
Sof(C) = 137.0 J/mol.K
Sof(D) = 200.0 J/mol.K
Balanced chemical equation is:
2 A + B ---> 2 C + 3 D
ΔSo rxn = 2*Sof(C) + 3*Sof(D) - 2*Sof( A) - 1*Sof(B)
ΔSo rxn = 2*(137.0) + 3*(200.0) - 2*(194.0) - 1*(183.0)
ΔSo rxn = 303 J/K
We have:
ΔHo = -147.0 KJ
ΔSo = 303 J/K
= 0.303 KJ/K
T = 306 K
use:
ΔGo = ΔHo - T*ΔSo
ΔGo = -147.0 - 306.0 * 0.303
ΔGo = -239.718 KJ
Answer: -240 KJ
Use the values from the table and calculate AGºrxn at 306 K in kJ. Enter the result no decimal places and no units....
Question 12 1 pts Use the values from the table and calculate AGºrxn at 306 K in kJ. Enter the result no decimal places and no units. 2A + 1B 2C + 3D compound AH®, kj/mol sºj/molK -78 194 -82 183 -80 137 -75 200
Use the values from the table and calculate ΔGorxn. in kJ. Enter the result with no decimal places and no units. 3A + 3B → 1C + 3D compound ΔGof kJ/mol A -38.8 B -93.7 C -19.1 D -75.6
Question 17 1 pts Use the values from the table and calculate the equilibrium constant kat 396 Kelvin. Enter the result with 3 s.f. and scientific notation. 1A + 1B → 2C + 1D compound B AGⓇkj/mol - 12.5 -14.4 - 11.9 -11.8
table 6
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction: NO2(g) + CO(g) + NO(g) + CO2(g) -990 kJ O-1211kJ O-420 kJ 0-199 kJ 0-222 kJ Table 6 (Cont.) - TI ΔΗ: sº (kJ/mol (J/kmol) AG; (kJ/moll at 25 H3(g) H2SO.) Hg) Ngo (3) 12 (8) K(s) KBr (5) KCl (S) KCIO, (s) KClO(S) KNO (3) Mg(s) MgCl2(s) MgCO3(s) Mgo(s) Mg(OH)2 (8) MgSO4(s) Mn(s) Mno(s) MnO2 (3) N2 (g) NH, (g) NH4Cl...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction: NO2(g) + CO(g) NO(g) + CO2(g) 0 -222 kJ 0-990 kJ 0 - 199 kJ O-1211 kJ O-420 kJ AG; (kJ/mol ) at 25°c AH; Sº (kJ/mol) (KJ/K mol) AG, (kJ/mol) at 25°c ΔΗ: sº (kJ/mol) (kJ/kmol) 0.0 -20.6 H2S (g) -33.6 +0.2057 -814.0 H2SO4(0) +0.1569 -690.1 0.0 Hg(e) 0.0 +0.0760 -90.8 Hgo (3) -58.6 +0.0703 12 () 0.0 0.0 +0.1161 0.0 K(s) +0.0642...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction: NO2(g) + CO(g) + NO(g) + CO2(g) O-420 kJ 0-222 kJ O-1211 kJ 0-199 kJ 0-990 kJ 3 pts Question 27 What is the pH of .731 M H2CO3 (aq)? 8.4 O 5.2 O 3.3 O 6.5 10.7 Table 6 - Thermodynamic Data of 12.0 M HOH ZOH is added to Ag(s) AgBr(s) Agcl(s) AgI (8) AgNO, () Ag20(8) Al(a) Al,0, () Ba (3)...
Use the data from this table of thermodynamic properties to calculate the values of ASixn for each reaction at 25 °C. 4NH,(g) + 70,(9) — 4NO2(g) + 6H2O(g) AS:n = J/mol K N,() + 0,(g) 2 NO(g) J/mol K Asian = MISU415) -1065.25 N2(9) N2H4(0) 50.6 N20(9) 81.6 N204(9) 11.1 N205(9) 13.3 NH3(9) -45.9 NH3(aq) -80.29 NH,+(aq) -133.3 NH4CI(S) -314.4 NH4NO3(s) -365.6 (NH2)2CO(s) -333.1 Na(s) Na+(aq) -240.3 Na2CO3(S) -1130.7 NaCl(s) -411.2 NaF(s) -576.6 NaBr(s) -361.1 Nal(s) -287.8 NaNO3(s) -467.9 NaOH(s)...
rates of chemical reactions
Plz help!! how do I find specific rate constant k, 1/T, In
K
thank you
Rates of Chemical Reactions: Report Form Rate Law Summary: (a) From your measurements, what are the reaction orders with respect to each of the three reactants H;O; HOO (b) What is the rate expression (rate law) for the uncatalyzed reaction? Rate = K LT-] [H202) (c) What is the total reaction order? 2 3. Effect of Temperature on the Reaction Rate...
only questions number: #3,6,8,16,19,22
Δι CH 122 - Practice Problems for Chapter 12 Do NOT use this problem set solely as test preparation. This problem set does NOT cover everything that we have discussed in class. You will still need to study class materials in order to do well on the learning assessment. 1. Of the following all are valid units for a reaction rate except A. moll B. M/S C. molhr D.g's E.molle 2. Which one of the following...