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Decomposition of Hydrogen Fluoride - General Chemistry
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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, GoTemperature

Consider the decomposition of hydrogen fluoride:

2HF(g) → H2(g) + F2(g)

Given that at 298KΔGo = 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 ΔSis 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?

Heart Capacity. Chemical Reaction General Chemistry - Exam


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)        ΔH= -802.34 kJ

Given that ΔHo(CO2) =-393.51 kJ and ΔHo(CH4)=-74.81 kJ, what is the ΔHfor 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) + 3H(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.