Question

For the reaction N2(g) + O2(g)2NO(g) H° = 181 kJ and S° = 24.9 J/K G° would be negative at temperatures (above, below) K. Enter above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant.

Answer 1

The formation of 2NO(g) from N2(g) and O2(g) has a ΔH° of 181 kJ. G° would be negative at temperatures above 7273.09 K.

Step-by-step explanation:

The reaction for the formation of 2NO(g) from N2(g) and O2(g) can be represented by the equation:

N2(g) + O2(g) → 2NO(g)

The enthalpy change for this reaction, ΔH°, is 181 kJ.

To determine whether the standard Gibbs free energy change, ΔG°, for the reaction is negative at a given temperature, we need to consider the equation:

ΔG° = ΔH° - TΔS°

If the value of ΔG° is negative, it means that the reaction is spontaneous and will proceed in the forward direction. This typically occurs at temperatures above a certain threshold, which is calculated using the equation ΔG° = 0.

For the given reaction, we can calculate the temperature at which ΔG° is negative by rearranging the equation:

T = (ΔH°) / (ΔS°)

Substituting the known values, we have:

T = 181 kJ / (24.9 J/K)

Converting kJ to J:

(T = 181,000 J) / (24.9 J/K) = 7273.09 K

Therefore, G° would be negative at temperatures above 7273.09 K.

Answer 2

ΔG deg will be negative above 7.27e+3 K.

Step-by-step explanation:

• The ΔG deg with the temperature can be found using the formula and the formula is given below
• ΔG deg = ΔH deg - T ΔS deg
• Given data, ΔH deg = 181kJ and ΔSdeg=24.9J/K
• -T ΔS deg will be always negative and ΔG deg = ΔH deg will be positive and ΔG deg will be negative at relatively high temperatures and positive at relatively low temperatures
• solving the equation and substitute ΔGdeg=0
• ΔGdeg = ΔHdeg - T ΔSdeg
• T= ΔHdeg/ΔSdeg
• T=181 kJ / 2.49e-2 kJK-1
• By simplification we get
• T=7.27 × 10^3 K.
• Therefore, Go will be negative above 7.27 × 10^3 K
• Since ΔG deg = -RT lnK, when ΔGdeg < 0, K > 1 so the reaction will have K > 1 above 7.27 × 10^3 K.

• ΔG deg will be negative above 7.27e+3 K.