A chemist fills a reaction vessel with 3.82 atm methanol (CH, OH) gas, 7.56 am oxygen (O2) gas, 5.29 atm carbon dioxide (CO2) gas, and 3.89 atm water (H0) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 2CH, OH() + 30266) 2002) + 4H20) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. x 5 ?

The Gibbs free energy of the given reaction is

Explanation:

The equation used to calculate Gibbs free energy change is of a reaction is:

For the given chemical reaction:

The equation for the Gibbs free energy change of the above reaction is:

We are given:

Putting values in above equation, we get:

The equation used to Gibbs free energy of the reaction follows:

where,

= free energy of the reaction

= standard Gibbs free energy = -1379.08 kJ/mol = -1379080 J/mol  (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314 J/K mol

T = Temperature =

= Ratio of concentration of products and reactants =

Putting values in above expression, we get:

Hence, the Gibbs free energy of the given reaction is

answer: at room temperature (roughly 20 degrees c), you can dissolve 203.9 grams (or 200 grams) of sugar in 100 ml of water. as water temperature increases, the amount of sugar that will dissolve increases, up to about 500 grams of sugar in 100 ml water at 100 degrees c.

explanation:

there all right good

explanation: