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podryga [215]
2 years ago
6

6.

Chemistry
1 answer:
RUDIKE [14]2 years ago
3 0

Answer:

THE CURRENT REQUIRED TO PRODUCE 193000 C OF ELECTRICITY IS 35.74 A.

Explanation:

Equation:

Al3+ + 3e- -------> Al

3 F of electricity is required to produce 1 mole of Al

3 F of electricity = 27 g of Al

If 18 g of aluminium was used, the quantity of electricity to be used up will be:

27 g of AL = 3 * 96500 C

18 G of Al = x C

x C = ( 3 * 96500 * 18 / 27)

x C = 193 000 C

For 18 g of Al to be produced, 193000 C of electricity is required.

To calculate the current required to produce 193 000 C quantity of electricity, we use:

Q = I t

Quantity of electricity = Current * time

193 00 = I * 1.50 * 60 * 60 seconds

I = 193 000 / 1.50 * 60 *60

I = 193 000 / 5400

I = 35.74 A

The cuurent required to produce 193,000 C of electricity by 18 g of aluminium is 35.74 A

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aksik [14]

Answer:

           The correct answer is Option-D (6 Hydrogen atoms).

Explanation:

                  Carbon atom has a unique property of linking to it self and making a chain of carbon called as Catenation. In a molecule having two carbon atoms there must be a bond between the two carbon atoms. The bond can be saturated (single bond) or unsaturated (double or triple bond). But as the statement states maximum number of hydrogen atoms so, we will asume the bond between two carbon atoms to be single.

                  As carbon has four valence electrons so, it has the ability to make four single bonds. In given molecule each carbon has already made a single bond with another carbon therefore, each carbon is left with three more unpaired electrons which will make covalent bond with three hydrogen atoms each as shown in attached structure.

8 0
2 years ago
Physical properties of glass bottle
Paul [167]
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8 0
2 years ago
If Co(NH3)63+ has a λmax at 440 nm, calculate ΔE for the complex. A) 2.72 x 10-4 kJ/mol B) 4.52 x 10-2 kJ/mol C) 2.72 x 10 2 kJ/
riadik2000 [5.3K]

<u>Answer:</u> The energy of the complex is 2.72\times 10^2kJ

<u>Explanation:</u>

To calculate the energy of the complex, we use the equation given by Planck which is:

\Delta E=\frac{N_Ahc}{\lambda}

where,

\lambda = Wavelength of the complex = 440nm=4.40\times 10^{-7}m    (Conversion factor:  1m=10^9nm )

h = Planck's constant = 6.624\times 10^{-34}Js

c = speed of light = 3\times 10^8m/s

N_A = Avogadro's number = 6.022\times 10^{23}

\Delta E = energy of the complex

Putting values in above equation, we get:

\Delta E=\frac{6.022\times 10^{23}\times 6.624\times 10^{-34}\times 3\times 10^8}{4.40\times 10^{-7}}\\\\\Delta E=2.72\times 10^{5}J=2.72\times 10^2kJ

Conversion factor used:  1 kJ = 1000 J

Hence, the energy of the complex is 2.72\times 10^2kJ

5 0
2 years ago
Acetaminophen (pictured) is a popular nonaspirin, "over-the-counter" pain reliever. what is the mass % (calculate to 4 significa
77julia77 [94]

Acetaminophen as a chemical formula of C8H9NO2. The molar masses are:

C8H9NO2 = 151.163 g/mol

C = 12 g/mol

H = 1 g/mol

N = 14 g/mol

O = 16 g/mol

 

<span>TO get the mass percent, simply multiply the molar mass of each elements  with the number of the element divide by the molar mass of acetaminophen, that is:</span>

%C = [(12 * 8) / 151.163] * 100% = 63.50%

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%N = [(14 * 1) / 151.163] * 100% = 9.262%

<span>%O = [(16 * 2) / 151.163] * 100% = 21.17% </span>

8 0
2 years ago
What mass of methanol is combusted in a reaction that produces 112 L of Co2 at STP?
AlekseyPX

Answer

D 160g

Explanation:

<u>Write the equation:</u>

Combustion reactions use oxygen and release water and heat, so

  CH₃OH(g) + O₂(g) → CO₂(g) + H₂O(g)

Balance that:

  2CH₃OH(g) + 3O₂(g) → 2CO₂(g) + 4H₂O(g)

<u>Find moles of carbon dioxide:</u>

We need to know the number of moles of CO₂. This rxn is at STP, so at STP one mole of gas = 22.4 liters.

  112 L * 1 mol/22.4 L = <em>5 mol CO₂</em>

<u>Find moles of methanol:</u>

Based on the chemical equation, for every 2 mol methanol, there are 2 mol carbon dioxide. So for every 5 mol carbon dioxide, there are 5 mol methanol!

  5 mol CO₂ = 5 mol CH₃OH

Molar mass of methanol: 12.01 + 3*1.008 + 16.00 + 1.008 = <em>32.04 g/mol</em>

Moles of methanol: 5 mol * 32.04 g/mol = 160.2 g methanol

≈ 160 mol methanol

8 0
2 years ago
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