A flask contains 0.25 mole of SO2(g), 0.50 mole of CH4(g), and 0.50 mole of O2(g). The total pressure of the gases in the flask

Response:

Examine the explanation

Explanation:

In this scenario, Nitrogen (N) experiences oxidation while Chlorine (Cl) undergoes reduction.

In response to your inquiry:

N is oxidized from an oxidation state of -3 to -1.

Cl is reduced from an oxidation state of +1 to -1.

At this point,

Borneol will likely exhibit a lower Rf due to its boiling point.

Answer: The change in enthalpy for each mole of zinc involved in the reaction is 152.4 kJ/mol.

Explanation:

First, we need to determine the moles of Zn and HCl.

The molar mass of Zn is 65 g/mole

and,

Next, we must identify the limiting reagent and the excess reagent.

The chemical reaction given is:

According to the balanced reaction we find that

1 mole of reacts with 2 moles of

Thus, 0.0206 moles of react with moles of

This leads us to determine that is the excess reagent because the moles provided exceed the required moles, while is limiting and restricts product formation.

Now to find the enthalpy change for each mole of zinc reacting in this reaction.

From the reaction we gather that,[ [TAG_59]]

0.0206 moles of Zn yield heat = 3.14 kJ

This implies that 1 mole of Zn generates heat =

Hence, the enthalpy change per mole of zinc involved in this reaction amounts to 152.4 kJ/mol.

Response:

Each molecule consists of one carbon atom.

9.837 * 10^24 molecules correspond to 9.837 * 10^24 carbon atoms.

It's a 1:1 relationship.