Chemical Reactions - Temperature and Gibbs Free Energy

1- If ΔH = -60.0kJ and ΔS = -0.200kJ/K , the reaction is spontaneous below a certain temperature. Calculate that temperature. Express your answer numerically in kelvins.

2-The chemical reaction that causes aluminum to corrode in air is given by
4Al+3O 2 →2Al 2 O 3 in which ΔH rxn ∘ = −3352 kJ and ΔS rxn ∘ = −625.1 J/K)

Part A: What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units.

Part B : What is the Gibbs free energy for this reaction at 5975K ? Assume that ΔH and ΔS do not change with temperature.Express your answer to two decimal places and include the appropriate units.

Part C: At what temperature, T , do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units.

Solution Summary

This solution contains detailed step-wise calculation of some numerical problems related to thermodynamics.

Focus Question: Consider a sample of CaO(s) at 298K and 1 atm. Does the Gibbsenergy of the sample increase, decrease of remain the same if the temperature is raised to 350K? Does the Gibbsenergy of the original sample increase, decrease of remain the same if the pressure is increased to 2 atm?
Important formula
1. For a co

What is Gibbsfreeenergy? What is the difference between entropy and enthalpy? What does the useful work derived do such that the entropy increases (additional to that increased along with enthalpy) but enthalpy remains the same (i.e the useful work does not increase the enthalpy)?

I completed part A and the second part asks:
What can be said about the spontaneity of this reaction?
C diamond to C graphite
The reaction (as written) is spontaneous.
The reverse reaction is spontaneous.
the system is in equilibrium at 298 K.

The change in G and the change in H are equal:
a. At O degrees Cesius
b. At O degrees K
c. When concentrations equal 1M and partal pressure equal 1 atm
d. When all reactants and products are in the same phase
e. When the reaction is exothermic

Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction
2 NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l)
Given that delta G^o = -13.6 kJ, calculate delta G at 25 oC for the following sets of conditions.
(a) 10 atm NH3, 10 atm CO2, 1.0 M NH2CONH2
(b) 0.1 atm NH3, 0.1 atm CO2, 1.0 M NH2CON

1- Calculate the change in Gibbsfreeenergy for each of the following sets of ΔH ∘ rxn , ΔS ∘ rxn , and T .
Part A : ΔH ∘ rxn =− 122kJ ; ΔS ∘ rxn = 248J/K ; T= 298K
Part B : ΔH ∘ rxn = 122kJ ; ΔS ∘ rxn =− 248J/K ; T= 298K
Part C : ΔH ∘ rxn =− 122kJ ; ΔS ∘ rxn =− 248J/K ; T=

1. Firstly, how do you calculate the molar solubility of AgBr when given 0.1 M AgBr at 25 degrees C (Ksp = 5 x 10^-3)?
If show me a few examples of how to calculate molar solubility when you're given different things, I would appreciate it.
2. Next, how can I calculate the squilibrium direction of CO2 at 25 degrees C and 9

The standard Gibbsfreeenergy of formation of NH3(g) is given by ∆Gfo=-16.5 kj/mol-1 at T=298K.
What is the Gibbsfreeenergy (∆G) for the reaction: N2(g) + 3H2 ↔ 2NH3(g) when the partial pressures are: PN2=3.0 bar; PH2=1.0 bar; and PNH3=4.0 bar?