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3 years ago

9

Which statement best explains the difference between polar and nonpolar covalent bonds?(1 point)

2 answers:

Mars2501 [29]3 years ago

8 0

Answer:

Let me help you out fr:

Explanation:

1. 0.5 to 1.7

2. fluorine (F)

3. KNO3

4. Polar covalent bonds share electrons unequally, while nonpolar covalent bonds share electrons equally.

5. Fe and S have an ionic bond, while S and O have covalent bonds.

miv72 [106K]3 years ago

6 0

Answer:

Answer is 4

Explanation:

Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms. ... If the electronegativity of two atoms is basically the same, a nonpolar covalent bond will form, and if the electronegativity is slightly different, a polar covalent bond will form.

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At 25 ∘C , the equilibrium partial pressures for the reaction were found to be PA=5.16 bar, PB=5.04 bar, PC=4.11 bar, and PD=4.8

erastova [34]

Answer: 5.85kJ/Kmol.

Explanation:

The balanced equilibrium reaction is

$A(g)+2B(g)\rightleftharpoons 4C(g)+D(g)$

The expression for equilibrium reaction will be,

$K_p=\frac{[p_{D}]\times [p_{C}]}^4{[p_{B}]^2\times [p_{A}]}$

Now put all the given values in this expression, we get the concentration of methane.

$K_p=\frac{(4.85)\times [(4.11)^4}{(5.04)^2\times (5.16)}$

$K_p=10.6$

Relation of standard change in Gibbs free energy and equilibrium constant is given by:

$\Delta G^o=-2.303\times RT\times \log K_c$

where,

R = universal gas constant = 8.314 J/K/mole

T = temperature = $25^0C=(25+273)K=298 K$

$K_c$ = equilibrium constant = 10.6

$\Delta G^o=-2.303\times 8.314\times 298\times \log (10.6)$

$\Delta G^o=5850.23J/Kmol$

$\Delta G^o=5.85kJ/Kmol$

Thus standard change in Gibbs free energy of this reaction is 5.85kJ/Kmol.

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