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3 years ago

How many moles of sulfate ions are in a sample of aluminum sulfate in which the number of formula units is 7.534 × 1023?

1 answer:

7 0

Answer:a unit of grammatical organization next below the sentence in rank and in traditional grammar said to consist of a subject and predicate

Explanation:

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C3H8 + 5O2 → 3CO2+ 4H2O, if 5.75L of oxygen are consumed in the above reaction, how many L of carbon dioxide are produced?

anzhelika [568]

Answer: 3.45 L carbon dioxide are produced

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given volume}}{\text {Molar volume}}=\frac{5.75L}{22.4L}=0.257moles$

$C_3H_8+5O_2(g)\rightarrow 3CO_2+4H_2O$

According to stoichiometry :

5 moles of $O_2$ produce = 3 moles of $CO_2$

Thus 0.257 moles of $O_2$ will produce= $\frac{3}{5}\times 0.257=0.154moles$ of $CO_2$

Volume of $CO_2=moles\times {\text {Molar volume}}=0.154moles\times 22.4L/mol=3.45$

Thus 3.45 L carbon dioxide are produced

6 0

3 years ago

When iron rusts in air iron3 oxide is produced. How many moles of oxygen react with 28.0 mol of iron in the rusting reaction 4fe

Marrrta [24]

This the balanced equation based on the question $4Fe + 3O_2 -\ \textgreater \ 2Fe_2O_3$ .

We then proceed with the following calculations

$28.0molFe*(\frac {3molO_2}{4mol Fe})= 21molO_2$

The answer is $21molO_2$ is produced.

5 0

3 years ago

In what situations are van der waals forces the most significant

viktelen [127]

Its most significant when all other forces are absent

7 0

3 years ago

An endergonic reaction with a Δh and Δs can be changed into an exergonic reaction.

zheka24 [161]

Full question:

This question is incomplete, here it is completed:

An endergonic reaction with a ______ ∆H and a ______ ∆S can be changed into an exergonic reaction by decreasing the temperature.

Option A: negative, positive

Option B: negative, negative

Option C: positive, positive

Option D: positive, negative

Answer:

Option B: negative, negative

Explanation:

The change in free energy (ΔG) of a system for a constant-temperature process is

ΔG = ΔH - TΔS

free energy is the energy available to do work. Thus, if a particular reaction is accompanied by a release of usable energy (that is, ΔG is negative), it is said to be exergonic. On the other hand, if a reaction consumes energy (that is, ΔG is positive), it is said to be endergonic.

Looking at the equation, we can see that if ΔH is negative and ΔS is negative, then ΔG will be negative only when TΔS is smaller in magnitude than ΔH. This condition is met when T is small.

ΔG = ΔH - TΔS

- -

This means that the reaction proceeds spontaneously at low temperatures. At high temperatures, the reverse reaction becomes spontaneous. An example of that would be the following reaction:

NH₃(g) + HCl(g) → NH₄Cl(s)

4 0

3 years ago

WILL MARK BRAINLIEST!! URGENT CORRECT ANSWERS NEEDED

atroni [7]

I hope this helps you;);

6 0

3 years ago