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3 years ago

Do hydrogen lose 1 2 or 3 electrons to other atoms

Chemistry

1 answer:

iren2701 [21]3 years ago

7 0

Answer: Hydrogen can lose as much as possible there is no limits to it.

Hope this helps!

I am joyous to assist you anytime!

-Jarvis

Extras: Hydrogen is the chemical element with the symbol H and atomic number 1. hydrogen is the lightest element in the periodic table. Hydrogen is the most abundant chemical substance in the Universe (;

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N204(0) + 2NO2(g)

user100 [1]

setup 1 : to the right

setup 2 : equilibrium

setup 3 : to the left

<h3>Further explanation</h3>

The reaction quotient (Q) : determine a reaction has reached equilibrium

For reaction :

aA+bB⇔cC+dD

$\tt Q=\dfrac{C]^c[D]^d}{[A]^a[B]^b}$

Comparing Q with K( the equilibrium constant) :

K is the product of ions in an equilibrium saturated state

Q is the product of the ion ions from the reacting substance

Q <K = solution has not occurred precipitation, the ratio of the products to reactants is less than the ratio at equilibrium. The reaction moved to the right (products)

Q = Ksp = saturated solution, exactly the precipitate will occur, the system at equilibrium

Q> K = sediment solution, the ratio of the products to reactants is greater than the ratio at equilibrium. The reaction moved to the left (reactants)

Keq = 6.16 x 10⁻³

Q for reaction N₂O₄(0) ⇒ 2NO₂(g)

$\tt Q=\dfrac{[NO_2]^2}{[N_2O_4]}$

Setup 1 :

$\tt Q=\dfrac{0.0064^2}{0.098}=0.000418=4.18\times 10^{-4}$

Q<K⇒The reaction moved to the right (products)

Setup 2 :

$\tt Q=\dfrac{0.0304^2}{0.15}=0.00616=6.16\times 10^{-3}$

Q=K⇒the system at equilibrium

Setup 3 :

$\tt Q=\dfrac{0.230^2}{0.420}=0.126$

Q>K⇒The reaction moved to the left (reactants)

8 0

2 years ago

Read 2 more answers

What type of soil has the most humus?

irinina [24]

Answer:

loamy soil

Explanation:

your welcome

4 0

2 years ago

How many formula units are present in 25.0 mol of sodium chloride

bonufazy [111]

The way to work out formula units is to do the amount of moles (in this case 25) times by 6.022 x 10^23. so, the answer is 1.5055 x 10^25 formula units. hope this helps! (by the way ^ represents ‘to the power of’ because i cant get the smaller symbols on here)

7 0

3 years ago

What would be the theoretical yield in grams of carbon dioxide in the reaction shown below if 30 g of C6H12O6 were reacted with

Vinvika [58]

Answer: Thus 44 g of $CO_2$ will be produced if 30 g of $C_6H_{12}O_6$ were reacted with an excess of oxygen

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} C_6H_{12}O_6 =\frac{30g}{180g/mol}=0.17moles$

The balanced chemical equation is:

$C_6H_{12}O_6 +6O_2(g)\rightarrow 6CO_2+6H_2O(g)$

As $C_6H_{12}O_6$ is the limiting reagent as it limits the formation of product and $O_2$ is the excess reagent.

According to stoichiometry :

1 mole of $C_6H_{12}O_6$ produce = 6 moles of $CO_2$

Thus 0.17 moles of $C_6H_{12}O_6$ will produce= $\frac{6}{1}\times 0.17=1.0mole$ of $CO_2$

Mass of $CO_2=moles\times {\text {Molar mass}}=1.0moles\times 44g/mol=44g$

Thus 44 g of $CO_2$ will be produced if 30 g of $C_6H_{12}O_6$ were reacted with an excess of oxygen.

8 0

3 years ago

Identify the oxidizing and reducing agents in the following: 2H+(aq) + H2O2(aq) + 2Fe2+(aq) → 2Fe3+(aq) + 2H2O(l)

schepotkina [342]

Answer : The oxidizing and reducing agents are, $H_2O_2$ and $Fe^{2+}$ .

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Reducing agent : It is defined as the agent which helps the other substance to reduce and itself gets oxidized. Thus, it will undergo oxidation reaction.

Oxidizing agent : It is defined as the agent which helps the other substance to oxidize and itself gets reduced. Thus, it will undergo reduction reaction.

The given redox reaction is:

$2H^+(aq)+H_2O_2(aq)+2Fe^{2+}(aq)\rightarrow 2Fe^{3+}(aq)+2H_2O(l)$

The half oxidation-reduction reactions are:

Oxidation reaction : $Fe^{2+}\rightarrow Fe^{3+}+1e^-$

Reduction reaction : $O^-+1e^-\rightarrow O^{2-}$

The oxidation state of oxygen in $H_2O_2$ and $H_2O$ is, (-1) and (-2) respectively.

In this reaction, 'Fe' is oxidized from oxidation (+2) to (+3) and 'O' is reduced from oxidation state (-1) to (-2). Hence, ' $Fe^{2+}$ ' act as a reducing agent and ' $H_2O_2$ ' act as a oxidizing agent.

Thus, the oxidizing and reducing agents are, $H_2O_2$ and $Fe^{2+}$ .

7 0

3 years ago