Areaction will be spontaneous only at low temperatures if both δh and δs are negative. for a reaction in which δh = −310.1 kj/mol and δs = −89.00 j/k · mol, determine the temperature (in °c) below which the reaction is spontaneous.

3211.12 K

Explanation:

The expression for the standard change in free energy is:

Where,  

is the change in the Gibbs free energy.

T is the absolute temperature. (T in kelvins)

is the enthalpy change of the reaction.

is the change in entropy.

For reaction to be spontaneous,

Given,

So,

Thus, applying values as:-

So, T = 3484.27 K

The conversion of T( °C) to T(K) is shown below:

T( °C)  = T(K) - 273.15  

So,  

T = (3484.27 - 273.15) K = 3211.12 K

The temperature below which the reaction is spontaneous is:- 3211.12 K

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.