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strojnjashka [21]
3 years ago
9

Fluorine is a gas and iodine is a solid, yet all halogens are non-polar and would interact with London dispersion forces. This i

s a result of​
Chemistry
1 answer:
attashe74 [19]3 years ago
6 0

Answer:

the molecules of each substance attract each other through dispersion (London) intermolecular force.whether a substance is solid, liquid or gas depends on the balance between the kinetic energies of the molecules and their intermolecular attractions.

thank you.

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Which reflects more sunlight-dark soil or white sand?
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I think the answer is white sand (sorry if i am wrong) 
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The equilibrium constant for the formation of ammonia from nitrogen and hydrogen is 1.6 × 102. what is the form of the equilibri
Nimfa-mama [501]

Answer: The expression for equilibrium constant is \frac{[NH_3]^2}{[H_2]^3[N_2]}

Explanation: Equilibrium constant is the expression which relates the concentration of products and reactants preset at equilibrium at constant temperature. It is represented as k_c

For a general reaction:

aA+bB\rightleftharpoons cC+dD

The equilibrium constant is written as:

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

Chemical reaction for the formation of ammonia is:

N_2+3H_3\rightleftharpoons 2NH_3

k_c=1.6\times 10^2

Expression for k_c is:

k_c=\frac{[NH_3]^2}{[H_2]^3[N_2]}

1.6\times 10^2=\frac{[NH_3]^2}{[H_2]^3[N_2]}

8 0
3 years ago
During the process of photosynthesis, green implants produce
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During photosynthesis, plants produce glucose from simple inorganic molecules - carbon dioxide and water - using light.
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3 years ago
@ What is the wavelength of a radio wave having a frequency of 3.75 X 107 Hz?
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2 years ago
G. Amount of charge required to reduce
Nady [450]

Answer:

\boxed{\text{c) 4 F}}

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NO₃⁻ ⟶ N₂O

2. Balance all atoms other than H and O

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5. Balance charge by adding electrons to the deficient side.

2NO₃⁻ + 10H⁺ + 8e⁻ ⟶ N₂O + 5H₂O

The amount of charge required to reduce 2 mol of NO₃⁻ is 8 F

\text{The amount of charge required to reduce 1 mol of NO$_{3}^{-}$ is \boxed{\textbf{4 F}}}

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3 years ago
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