What is the ΔG for the following reaction at 25°C?

2 answers:

5 0

The ΔG for the following reaction at 25°C of N2O4(g) → 2NO2(g) is 5.32 kJ per mole.

2 (51.8) - 98.28 = 5.32 kJ per mole.

This is because the rate of the dissociation of N2O4 is equal to the rate of formation of N2O4.

ikadub [295]2 years ago

4 0

$\Delta G_{global}=\Delta G_{products}-\Delta G_{reagents}\\\\
\text{We should consider the stoichiometry:}\\\\
\Delta G=2\Delta G_{NO_2}-\Delta G_{N_2O_4}\\\\
\Delta G=2\cdot51.8-98.28=103.6-98.28\\\\
\boxed{\Delta G=5.32~kJ}$

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Write the nuclear equation to describe the alpha decay of 243 95 Am

motikmotik

Answer:

Here's what I get.

Explanation:

Your unbalanced nuclear equation is:

$_{95}^{243}\text{Am} \longrightarrow \, _{x}^{y}\text{Z} +\, _{2}^{4}\text{He}$

The main point to remember in balancing nuclear equations is that the sums of the superscripts and the subscripts must be the same on each side of the equation.

Then

95 = x + 2, so x = 95 - 2 = 93

243 = y + 4, so y = 243 - 4 = 239

Element 93 is neptunium, so the nuclear equation becomes

$_{95}^{243}\text{Am} \longrightarrow \, _{93}^{239}\text{Np} + \, _{2}^{4}\text{He}$