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Mekhanik [1.2K]
3 years ago
12

What are the structures in which stars are grouped together?

Chemistry
1 answer:
disa [49]3 years ago
4 0

Answer:

constellations

Explanation:

You might be interested in
Which functional group does the molecule below have?
Andrei [34K]

Answer:

Hydroxyl

Explanation:

A hydroxyl group is a functional group that attaches to some molecules containing an oxygen and hydrogen atom, bonded together. Also spelled hydroxy, this functional group provides important functions to both alcohols and carboxylic acids.

3 0
3 years ago
One application of Hess's Law (which works for ΔH, ΔS, and ΔG) is calculating the overall energy of a reaction using standard en
VikaD [51]

Answer:

The standard change in free energy for the reaction =  - 437.5 kj/mole

Explanation:

The standard change in free energy for the reaction:

                              4 KClO₃ (s) → 3 KClO₄(s) + KCl(s)

Given that   ΔGf(KClO3(s)) = -290.9 kJ/mol;

                    ΔGf(KClO4(s)) = -300.4 kJ/mol;

                    ΔGf(KCl(s)) = -409 kJ/mol

According to Hess's law

ΔGr (Free energy change of reaction)= ∑(Product free energy - reactant free energy)

               ⇒ ΔGr⁰ = {3 x (-300.4) + (-409)} - {3 x (- 290.9)}

                            = - 901.2 - 409 + 872.7

                            =  - 437.5 kj/mole

3 0
3 years ago
About _% of high school seniors report misusing prescription
mihalych1998 [28]
About 5% of high school seniors reportmisusing prescription
5 0
3 years ago
At room temperature, a melting solid produces a whitish liquid. A laser beam shined through the liquid is unaffected and produce
navik [9.2K]
The answer is a colloid.
8 0
3 years ago
The enthalpy of a pure liquid at 75oC is 100 J/mol. The enthalpy of the pure vapor of that substance at 75oC is 1000 J/mol. What
pentagon [3]

Answer:

900 J/mol

Explanation:

Data provided:

Enthalpy of the pure liquid at 75° C = 100 J/mol

Enthalpy of the pure vapor at 75° C = 1000 J/mol

Now,

the heat of vaporization is the the change in enthalpy from the liquid state to the vapor stage.

Thus, mathematically,

The heat of vaporization at 75° C

=  Enthalpy of the pure vapor at 75° C - Enthalpy of the pure liquid at 75° C

on substituting the values, we get

The heat of vaporization at 75° C = 1000 J/mol - 100 J/mol

or

The heat of vaporization at 75° C = 900 J/mol

8 0
3 years ago
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