For the sublimation of iodine at 25C
I2(s) yield I2(g)
the values of H and G are, respectively, 62 kJ and 19 kJ. Estimate the temperature at which iodine sublimes. Assume H and S do not depend on temperature.
Given,
For the sublimation reaction of iodine at 25°C
standard enthalpy, ΔH = 62 kJ = 62000 J
standard free energy ΔG = 19 kJ = 19000 J
T = 273.15 + 25 = 298.15 K
Using these values and below formula, calculate the standard entropy of 25°C
ΔG = ΔH-TΔS
19000 J = 62000 J - (298.15 K)ΔS
ΔS = (62000 -19000)J/(298.15)K
ΔS = 144.22 J/K
Calculate the temperature for the sublimation of iodine using following formula
T = ΔH/ΔS
T = (62000 J)/(144.22 J/K)
T = 429.9 K
T = 429.9-273.15 = 156.8°C
Temperature for sublimation of iodine = 156.8°C or 429.9 K
For the sublimation of iodine at 25C I2(s) yield I2(g) the values of H and G...
Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. (a) What is the half-life for this reaction? _______ s (b) If you start with 0.051 M I2 at this temperature, how much will remain after 5.30 s assuming that the iodine atoms do not recombine to form I2? _______ M
Using the following information, calculate the heat of sublimation of S(s) to S(g). ?H°f MgS= -343 kJ/mol, ?H°sublimation Mg(s) = 148 kJ/mol, The lattice energy MgS = 3406 kJ/mol ?Mg(g) ? Mg2+(g) + 2 e ??st + 2nd IE = 2186 kJ/mol, S(g) +2e ? S2-(g) ????H = 450 kJ/mol, A. 575 kJ/mol B. 1179 kJ/mol C. 279 kJ/mol D. 965 kJ/mol E. 4651 kJ/mol
Titanium reacts with iodine to form titanium(III) iodide, emitting heat: 2 Ti(s) + 3 I2(g) → 2 TiI3(s) ΔH°rxn = −839 kJ Determine the masses of titanium and iodine that react if 1.55×103 kJ of heat is emitted by the reaction.
Molecular iodine, I2 (g), dissociates into iodine
atoms at 652 K, with a first order rate constant of 0.452
s-1.
a. What is the half life for this reaction?
[ Select ]
["1.53 s", "0.31 s", "0.079 s", "0.39 s"]
b. If you start with 0.35 M I2 at this temperature,
how long will it take for the concentration of I2 to
reach...
What is
G at 298 K for I2(g) + Cl2(g)
2ICl(g);
H= -27.4 kJ;
S= 11.5 J?
The reaction H2(g) + I2(g) → 2 HI (g) is first order in both hydrogen and iodine. It is therefore referred to as second order overall. Its rate constant for the formation of HI (g) at 400 ◦C is 2.34 × 10−2 · lit · mol−1 · sec−1 and its activation energy is 150 KJ/mol. Use the rate law to estimate how long it takes to form 0.1 mole of HI(g) if I start by putting 2 moles of H2...
Data is for P 1 bar and 25C AH (kJ mol) NAg) H,(g) NH (g) S (J K mol ) 191.5 130.6 192.3 46.1 13) 812. (a) Calculate &G" for the tollawing reaction at 25 C. Ng) 3 H,(g) 2 NH,1g) (b) Account for the sign of &s. Give your reasoning Calculate the value of K-or the reaction at 3000'C. assumptions required 13] (c) State any 12) id) Calculate 4at 30 0 Cwhen PIN)- 300 bar P)1200 bar and P(NH,1-0.0010...
16. The sublimation of carbon dioxide at -78°C is given by: CO2(8) = CO2(g) AHsub = 25.2 kJ/mol Calculate ASsub when 48.8 g of CO2 sublimes at this temperature AH-26.23 A) 330 J/K B) 143 J/K C) 249 J/K D) 129 J/K E) 79.6 JK 17. A galvanic cell consists of a silver electrode in contact with 0.100 M AgNO3 solution and a magnesium electrode in contact with 0.100 M Mg(NO3)2 solution. Calculate the potential, Ecell, at 25°C. Given: Ag...
The data in the table above were determined at 25C.
(a) Calculate G for the reaction above at 25C.
(b) Calculate Keq for the reaction above at 25C.
(c) Calculate S for the reaction above at 25C.
(d) In the table above, there are no data for H2. What are the
values of Hf, Gf, and of the absolute entropy, S, for H2 at
25C?
Using Equilibrium Constants to Determine Thermodynamic Parameters Post Lab So AHP (kJ mol (kJmol (J...
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