Decomposition, Hydrogen Fluoride, Spontaneous, Reaction – General Chemistry Exam
The key terms in this Chemistry course include Decomposition, Hydrogen Fluoride, Spontaneous, Reaction, Enthalpical, Entropical, Endothermic, Heat, Metals, Sample, ∆Ho, ∆So, Equilibrium Constant, Heat Capacity, Alloy, Haber process, Ammonia, ∆Go, Temperature
Consider the decomposition of hydrogen fluoride:
2HF(g) → H2(g) + F2(g)
Given that at 298K, ΔGo = 38.3 kJ, [HF] = 0.070 atm, [H2] = 0.025 atm and [F2] = 0.0035atm, which of the following statements about this reaction at 298K is correct?
Under these conditions Q > K and the reaction will be spontaneous in the reverse direction.
Is the following reaction enthalpically or entropically driven?
2SO3(g) → 2SO2(g) + O2(g) ΔH = 198.2 kJ
Entropically driven because it is endothermic and ΔSo is positive.
If I add 100 kJ of heat to a 50.0 g sample of each of the following metals, which one will heat up the most slowly?
Given that at 298K for the reaction A3 + 6B → 3AB2 ΔHo = 75 kJ/mol, what is the ΔHo value for the reaction AB2 → (1/3)A3 + 2B?
-25 kJ/mol
Without doing any calculations, predict the signs of ∆Ho, ∆S˚, ∆HSURRo, ∆SSURR˚ and ∆Go for the reaction:
A(g) + B(g) → AB(g)
∆Ho < 0, ∆So < 0, ∆HSURRo > 0, ∆SSURRo > 0 and ∆Go is unknown
Consider the following reaction:
2H2(g) + O2(g) → 2H2O(g) ΔHo = -484 kJ/mol
If you react 0.80 mol of H2(g) and 0.60 mol of O2(g), what is the heat for the reaction?
-194 kJ
Consider the following reaction:
C2H4(g) + H2O(g) ⇌ C2H5OH(g) ΔHo = -45.8 kJ/mol
At 298K the equilibrium constant, KP, for this reaction is 28.5. What is ΔG for this reaction at 298K under the following conditions: p(C2H4) = p(H2O) = p(C2H5OH) = 3.0 atm?
-11.0 kJ/mol
Consider the following reaction:
CH4(g) + 2O2(g) → 2H2O(g) + CO2(g) ΔHo = -802.34 kJ
Given that ΔHo(CO2) =-393.51 kJ and ΔHo(CH4)=-74.81 kJ, what is the ΔHo for H2O?
-241.82 kJ
In an experiment 359 J of heat were spent to raise the temperature of a 57.0 g sample of an unknown alloy by 54.0oC. What is the heat capacity of this alloy?
0.117 J/g- oC
Consider the Haber process for the production of ammonia:
N2(g) + 3H2 (g) →2NH3(g)
This reaction is thermodynamically spontaneous at 298K, but becomes nonspontaneous at higher temperatures. Which of the following statements is true about this reaction under standard conditions at 298K?
∆Go, ∆Ho, and ∆So are all negative.