## N2 + 2H2 ==> N2H4

dGrxn = (n*dGf products) - (n*dGf reactants).

According to my tables N2H4 is -16 kJ/mol, N2 and H2 are zero.

You need to use the numbers in your tables.

N2(g) + H2(g) right arrow N2H4(l)

DrBob222
answered

11 years ago

11 years ago

dGrxn = (n*dGf products) - (n*dGf reactants).

According to my tables N2H4 is -16 kJ/mol, N2 and H2 are zero.

You need to use the numbers in your tables.

Explain Bot
answered

11 months ago

11 months ago

The standard free-energy change can be calculated using the equation:

Î”GÂ° = âˆ‘nÎ”GÂ°f(products) - âˆ‘nÎ”GÂ°f(reactants)

Where âˆ‘nÎ”GÂ°f(products) is the sum of the standard free-energy change of formation for each product, and âˆ‘nÎ”GÂ°f(reactants) is the sum of the standard free-energy change of formation for each reactant.

First, you need to determine the Î”GÂ°f values for each species involved in the reaction. You can find these values in tables or databases of thermodynamic data.

Using the given reaction:

N2(g) + H2(g) â†’ N2H4(l)

Here are the Î”GÂ°f values for each species:

Î”GÂ°f(N2(g)) = 0 (since it is in its standard state)

Î”GÂ°f(H2(g)) = 0 (since it is in its standard state)

Î”GÂ°f(N2H4(l)) = 50.6 kJ/mol

Now substitute these values into the equation to solve for Î”GÂ°:

Î”GÂ° = (1 Ã— Î”GÂ°f(N2H4(l))) - (1 Ã— Î”GÂ°f(N2(g))) - (1 Ã— Î”GÂ°f(H2(g)))

Î”GÂ° = (1 Ã— 50.6 kJ/mol) - (1 Ã— 0 kJ/mol) - (1 Ã— 0 kJ/mol)

Î”GÂ° = 50.6 kJ/mol

Therefore, the standard free-energy change for the synthesis of hydrazine from nitrogen and hydrogen is 50.6 kJ/mol.