Estimate Keq for the following equilibria at 350 K. R = 8.3145
J/(mol*K). Substance ΔHo(kJ/mol) So(J/(mol*K)) SnO2(s) -577.6 49.0
H2(g) 0 130.680 CO(g) -110.5 197.7 Sn(s, white) 0 51.2 H2O(l)
-285.83 69.95 Fe(s) 0 27.3 Fe3O4(s) -1118.4 146.4 Correct answer.
Correct. SnO2(s) + 2H2(g) ⇄ Sn(s, white) + 2H2O(l) The number of
significant digits is set to 2; the tolerance is +/-3% LINK TO TEXT
Incorrect answer. Incorrect. 3Fe(s) + 4H2O(l) ⇄ Fe3O4(s) + 4H2(g)
Entry field with incorrect answer...
Suppose Delta G^o is 25.0 KJ/mol for a hypothetical
reaction in which A converts into B. Which of the following
statements describes an equlibrium mixture of A and B?
a) B has a higher concentration than A.
b) Only A is present.
c) A and B have equal concentrations.
d) Only B is present.
e) A has a higher concentration than B.
Could you please explain your reasoning behind the
answer as well?
For the reaction below, Δ S ° = − 269 J/(mol · K) and Δ H ° = −
103.8 kJ/mol. Calculate the equilibrium constant at 25 °C.
3C(s) + 4H_2 (g) -->C_3+ H_8 (g)
For a given reaction, the heat capacity (CP) of the reactants is
50.0 J/mol K and for the products is 65.0 J/mol K. If the enthalpy
of reaction is − 150.0 kJ/mol at 300K, what is the best
estimate of ΔrxnH at 320K?
The reaction in the previous question is carried out
adiabatically starting at 300 K. What is the final
temperature after the reaction goes to completion?
ΔrxnH300 = -150.0 kJ/mol
CP(reactants) = 50 J/molK
CP(products) = 65 J/molK...
For a particular reaction at 215.7 °C, ΔG = 404.91 kJ/mol, and
ΔS = 748.20 J/(mol·K).
Calculate delta G for -74.3 celcius.
I've asked this question previously and the individual who
answered got roughly 378 kj/mol which is incorrect.
The reaction
C4H8(g)⟶2C2H4(g)C4H8(g)⟶2C2H4(g)
has an activation energy of 262 kJ/mol.262 kJ/mol. At 600.0
K,600.0 K, the rate constant, ?,k, is 6.1×10−8 s−1.6.1×10−8 s−1.
What is the value of the rate constant at 765.0 K?