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lara31 [8.8K]
3 years ago
14

In the Lewis structure of the iodate ion, IO3 – , that satisfies the octet rule, the formal charge on the central iodine atom is

A) +2 B) +1 C) 0 D) –1 E) –2
Chemistry
1 answer:
vitfil [10]3 years ago
6 0

Answer:

- 1 is the correct option

Explanation:

In determining the oxidation state or formal charge on element in an ionic specie, the whole ion need to be equated to the value of charge on the ion.

For example in this case, the charge on the ion is -3. Thus; representing iodine with X and putting -2 for the oxidation state of O (oxygen)

X + -2 = -3 (adding 2 to both side)

X = -3 + 2

X = - 1

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Find the equilibrium value of [CO] if Kc=14.5 : CO (g) + 2H2 (g) ↔ CH3OH (g) Equilibrium concentrations: [H2] = 0.322 M and [CH3
Annette [7]

Answer:

The equilibrium value of [CO] is 1.04 M

Explanation:

Chemical equilibrium is the state to which a spontaneously evolving  chemical system, in which a reversible chemical reaction takes place.  When this situation is reached, it is observed that the  concentrations of substances, both reagents and reaction products,  they remain constant over time. That is, the rate of reaction of reagents to products is the same as that of products to reagents.

Reagent concentrations  and products in equilibrium are related by the equilibrium constant Kc. Being:

aA + bB ⇔ cC + dD

Kc=\frac{[C]^{c} *[D]^{d} }{[A]^{a} *[B]^{b} }

Then this constant Kces equals the multiplication of the concentrations of the products raised to their stoichiometric coefficients between the multiplication of the concentrations of the reactants also raised to their stoichiometric coefficients.

In this case:

Kc=\frac{[CH_{3}OH ]}{[CO]*[H_{2} ]^{2} }

You know:

  • Kc= 14.5
  • [H₂]= 0.322 M
  • [CH₃OH] =1.56 M

Replacing:

14.5=\frac{1.56}{[CO]*0.322^{2} }

Solving:

[CO]=\frac{1.56}{14.5*0.322^{2} }

[CO]= 1.04 M

The equilibrium value of [CO] is 1.04 M

8 0
3 years ago
What phase of matter is oxygen at room temperature
Vedmedyk [2.9K]
Gas

good luck mate :)
8 0
2 years ago
3. (01.03 MC)
sleet_krkn [62]

The majority of wind turbines consist of three blades mounted to a tower made from tubular steel. There are less common varieties with two blades, or with concrete or steel lattice towers. At 100 feet or more above the ground, the tower allows the turbine to take advantage of faster wind speeds found at higher altitudes.

Turbines catch the wind's energy with their propeller-like blades, which act much like an airplane wing. When the wind blows, a pocket of low-pressure air forms on one side of the blade. The low-pressure air pocket then pulls the blade toward it, causing the rotor to turn. This is called lift. The force of the lift is much stronger than the wind's force against the front side of the blade, which is called drag. The combination of lift and drag causes the rotor to spin like a propeller. So therefore your answer would be A.

If this helped could you leave a brainlyest?

8 0
3 years ago
it takes 513 kj to remove a mole of electrons from the atoms at the surface of a piece of metal. how much energy does it take to
schepotkina [342]

Answer:

The right solution is "8.5\times 10^{-19} \ joule".

Explanation:

As we know,

1 mole electron = 6.023\times 10^{23} \ no. \ of \ electrons

Total energy = 513 \ KJ

                     = 513\times 1000 \ joule

For single electron,

The amount of energy will be:

= \frac{513\times 1000}{(6.023\times 10^{23})}

= 8.5\times 10^{-19} \ joule

8 0
3 years ago
Given the balanced equation below, calculate the moles of aluminum that are needed to react completely with 28.7 moles of FeO. Y
Alexxx [7]

Answer:

43.05 moles of Al needed to react with 28.7 moles of FeO.

Explanation:

Given data:

Moles of FeO = 28.7 mol

Moles of Al needed to react with FeO = ?

Solution:

Chemical equation:

2Al + 3FeO → 3Fe + Al₂O₃

Now we will compare the moles of Al with FeO.

                            FeO        :           Al

                             2            :            3

                          28.7          :         3/2×28.7 = 43.05 mol

Thus 43.05 moles of Al needed to react with 28.7 moles of FeO.

8 0
3 years ago
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