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Nesterboy [21]
2 years ago
11

How many moles of H2O are needed to react with a mole of 3.0 of Na?​

Chemistry
1 answer:
AveGali [126]2 years ago
5 0

Answer: 3.0 moles of water (H_2O)  are needed to react with a mole of 3.0 of Na

Explanation:

The balanced chemical reaction of sodium with water is as follows:

2Na+2H_2O\rightarrow 2NaOH+H_2

According to stoichiometry:

2 moles of sodium (Na) reacts with = 2 moles of water (H_2O)

Thus 3.0 moles of sodium (Na) reacts with = \frac{2}{2}\times 3.0=3.0 moles of water (H_2O)

3.0 moles of water (H_2O)  are needed to react with a mole of 3.0 of Na

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An electromagnet is a device in which, by electric current, the magnetic field is produced. Increase the number of coils and increase the strength of the current, thus, increasing the strength of an electromagnet.

The correct option is B.

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Wherever controllable magnets are required, such as in devices where the magnetic flux must be adjusted, reversed, or switched on and off, an electromagnet is utilized.

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2 years ago
The value of Ka for nitrous acid (HNO2) at 25 ∘C is 4.5×10−4 .a. Write the chemical equation for the equilibrium that correspond
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Answers and Explanation:

a)- The chemical equation for the corresponden equilibrium of Ka1 is:

2. HNO2(aq)⇌H+(aq)+NO−2

Because Ka1 correspond to a dissociation equilibrium. Nitrous acid (HNO₂) losses a proton (H⁺) and gives the monovalent anion NO₂⁻.

b)- The relation between Ka and the free energy change (ΔG) is given by the following equation:

ΔG= ΔGº + RT ln Q

Where T is the temperature (T= 25ºc= 298 K) and R is the gases constant (8.314 J/K.mol)

At the equilibrium: ΔG=0 and Q= Ka. So, we can calculate ΔGº by introducing the value of Ka:

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  ΔGº= 19092.8 J/mol

c)- According to the previous demonstation, at equilibrium ΔG= 0.

d)- In a non-equilibrium condition, we have Q which is calculated with the concentrations of products and reactions in a non equilibrium state:

ΔG= ΔGº + RT ln Q

Q= ((H⁺) (NO₂⁻))/(HNO₂)

Q= ( (5.9 10⁻² M) x (6.7 10⁻⁴ M) ) / (0.21 M)

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We know that   ΔGº= 19092.8 J/mol, so:

ΔG= ΔGº + RT ln Q

ΔG= 19092.8 J/mol + (8.314 J/K.mol x 298 K x ln (1.88 10⁻⁴)

ΔG= -2162.4 J/mol

Notice that ΔG<0, so the process is spontaneous in that direction.

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Answer:

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