Areaction will be spontaneous only at low temperatures if both δh and δs are negative. for a reaction in which δh = −320.1 kj/mol and δs = −98.00 j/k · mol, determine the temperature (in °c) below which the reaction is spontaneous.

2993 °C

Explanation:

A reaction is spontaneous if the free Gibbs energy (ΔG) is negative. ΔG is related to the enthalpy of the reaction (ΔH) and the entropy of the reaction (ΔS) through the following expression.

ΔG = ΔH - T . ΔS

For 1 mol, if ΔG < 0, then

ΔH - T . ΔS < 0

ΔH < T . ΔS

-320.1 × 10³ J < T . (-98.00 J/K)

T < 3266 K

To convert Kelvin to Celsius we use the following expression.

K = °C + 273.15

°C = K - 273.15 = 3266 - 273.15 = 2993 °C

increasing transnational kinetic energy. because the transnational kinetic energy formula consists of only two variables, mass and velocity, increasing one of those properties is the only way to increase an object's transnational kinetic energy. increases to mass and velocity, however, do not have the same impact.

neither accurate nor precise.