For the reaction below

2 CH3OH(l) + 3 O2(g) 2 CO2(g) + 4 H2O(g)
calculate Srxn at 298 K.

(Hint: Use a table of thermodynamic data commonly found at the back of chemistry textbooks.)

To calculate the entropy change (ΔSrxn) for the given reaction at 298 K, you will need the standard entropy values for each of the compounds involved in the reaction. These values can be found in a table of thermodynamic data.

Using the data from the table, you can calculate the entropy change as follows:

1. Identify the standard entropy value (S°) for each compound involved in the reaction. For this reaction, you need the standard entropy values for CH3OH(l), O2(g), CO2(g), and H2O(g).

2. Multiply the standard entropy value (S°) of each compound by the stoichiometric coefficient of that compound in the balanced equation. This accounts for the number of moles of that compound participating in the reaction.

For the given reaction:

2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)

The stoichiometric coefficients are:

CH3OH(l): 2
O2(g): 3
CO2(g): 2
H2O(g): 4

3. Calculate the total entropy change by summing up the products and subtracting the sum of the reactants:

ΔSrxn = (2 × S°(CO2(g))) + (4 × S°(H2O(g))) - (2 × S°(CH3OH(l))) - (3 × S°(O2(g)))

Substitute the values of the standard entropy (S°) from the table for each compound, and perform the calculations to find the total entropy change (ΔSrxn) at 298 K.

To calculate the standard entropy change (ΔSrxn) for the given reaction at 298 K, we will need to use the thermodynamic data commonly found in the back of chemistry textbooks.

The standard entropy change for a reaction can be calculated using the following equation:

ΔSrxn = ∑nS°(products) - ∑mS°(reactants)

where ΔSrxn is the standard entropy change, n is the stoichiometric coefficient of the products, S°(products) is the standard entropy of the products, m is the stoichiometric coefficient of the reactants, and S°(reactants) is the standard entropy of the reactants.

For the given reaction:
2 CH3OH(l) + 3 O2(g) -> 2 CO2(g) + 4 H2O(g)

We need to find the standard entropy values for each species involved in the reaction.

You can find these values in a table of thermodynamic data, often provided in the back of chemistry textbooks. Look for the standard entropy (S°) values for CH3OH(l), O2(g), CO2(g), and H2O(g).

Once you have the standard entropy values for each species, substitute these values into the equation to calculate ΔSrxn. Remember to account for the stoichiometric coefficients when calculating the entropy change for each reactant and product.

delta S rxn = (n*DS products) - (n*DS reactants).

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