a) Is the following reaction spontaneous at standard reaction
conditions?
b) At what temperature (oC) does the reaction become
spontaneous?
CaCO3(s) --> CaO(s) + CO2(g)
What is the condition for a reaction to be spontaneous? If a
reaction is spontaneous at one temperature is it spontaneous under
all conditions? [10 marks] ii) Given the following information
?fH°(CH3OH(g)) = -201.0 kJ mol-1 / S°(CH3OH(g)) = 239.70 J mol-1
K-1 ?fH°(CH2O(g)) = -108.6 kJ mol-1 / S°(CH2O(g)) = 218.95 J mol-1
K-1 ?fH°(H2(g)) = 0 / S°(H2(g)) = 130.70 J mol-1 K-1 determine
?rH°, ?rS° and ?rG° for the formation of formaldehyde from the
dehydrogenation of methanol...
Which of the following definitively describes a spontaneous
process?
a. -delta G
b. - delta H
c. + delta H
d. + delta G
Which of the following statements is true
a. exothermic processes decrease the entropy of the
surroundings
b. none are true
c. deltaSuniv is always decreasing for spontaneous process
d. free atoms have greater entropy than molecules
What is an option delta? If delta is 0.5 what does this mean?
How does delta change when the option is in-the-money,
at-the-money, and out-of-the-money
Which of the following are true for a spontaneous process in a
system at constant temperature and pressure? I. ∆Ssys + ∆Ssurr >
0 II. ∆Gsys < 0 It is possible both or neither could be true, or
just one.
What does it mean for a free energy diagram of an equilibrium
reaction when delta G is zero? Does that mean that the entire
diagram would just be a horizontal line, or would there still be
transition and intermediate states?
What does it mean if delta G naught is higher at low temperature
(5 degrees celsius) and lower at high temperature( 25 degree
celsius or room temp) but delta S naught is the same at both
temperatures? Ksp was also lower at low temp and higher at high
temp.
Details: Is this as it should be and if so please explain why.
All values are positive. Delta G naught= 19.19 kJ/mol at room temp
and 23.66 kJ/mol at 5 degrees....