The above reaction is used in the industrial production of hydrogen cyanide. Con

Question

The above reaction is used in the industrial production of hydrogen cyanide. Consider the relevant thermodynamic data from the appendices of your text. (The tabulated values H°f and S° are for 25°C. For the purposes of this question assume that H° and S° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)

So I calculated H° and S° and G° and it's -939.8 kJ, 165 J/K , and -990.3 kJ .

Now I need help answering these True/False questions. I'm on my last try so I hope someone can answer them correctly.

Are the following statements about this process True or False?

The high temperature required for this process is needed for kinetic reasons.
This reaction is exothermic at 1000°C.
The equilibrium position for this reaction is further to the left at higher temperatures.
Thermodynamically, this reaction is spontaneous at any temperature.
At temperatures significantly lower than 1000°C this reaction is spontaneous.

Explanation / Answer

1) The high temperature required for this process is needed for kinetic reasons. (True)

2) This reaction is exothermic at 1000°C. (True)

3) The equilibrium position for this reaction is further to the left at higher temperatures. (True)

4) Thermodynamically, this reaction is spontaneous at any temperature.(False)

5) At temperatures significantly lower than 1000°C this reaction is spontaneous. (false)

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