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2 years ago

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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What is the maximum number of hydrogen atoms that can be covalently bonded in a molecule containing two carbon atoms?a) 2b) 3c)

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Answer:

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

Explanation:

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2 years ago

Physical properties of glass bottle

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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]

Answer: The energy of the complex is $2.72\times 10^2kJ$

Explanation:

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 $2.72\times 10^2kJ$

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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

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:

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

%H = [(1 * 9) / 151.163] * 100% = 5.954%

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

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

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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:

Write the equation:

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)

Find moles of carbon dioxide:

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 = 5 mol CO₂

Find moles of methanol:

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 = 32.04 g/mol

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

≈ 160 mol methanol

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