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4 years ago

How many grams of NH3 are needed to provide the same number of molecules as in 0.15 grams of SF6

1 answer:

3 0

Moles of SF6 = 0.15/molar mass of SF6 = 0.15/146.06 = 1.02 x 10⁻³ moles.
Moles of NH3 = Moles of SF6 = 1.02 x 10⁻³ moles.

Therefore mass of NH3 = moles of NH3 x molar mass of NH3
= 1.02 x 10⁻³ x 17.03
= 0.017 grams.

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Why is water a polar molecule? ? Why is water a polar molecule? ? 4 following 6 answers 6 Report Abuse Are you sure you want to

anyanavicka [17]

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3 years ago

Identify the oxidizing and reducing agent in the following reaction, and determine which element is oxidized and which is reduce

erma4kov [3.2K]

Answer:

Explanation:

Fe⁺²(aq) + ClO₂(aq) → Fe⁺³(aq) + ClO₂⁻(aq)

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The oxidation number of Cl is reduced from + 4 to +3 so Cl is reduced .

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3 years ago

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3 years ago

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Harman [31]

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3 years ago

For the following electrochemical reaction: Al3+(aq) + 3e -> Al(s) Eº = -1.66 V E° = 2.87 F2(g) + 2e -> 2F (aq) Calculate

makvit [3.9K]

Answer: The standard electrode potential of the cell is 4.53 V.

Explanation:

We are given:

$E^o_{(F_2/F^-)}=2.87V\\E^o_{(Al^{3+}/Al)}=-1.66V$

The substance having highest positive $E^o$ potential will always get reduced and will undergo reduction reaction. Here, fluorine will undergo reduction reaction will get reduced.

Aluminium will undergo oxidation reaction and will get oxidized.

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

$E^o_{cell}=2.87-(-1.66)=4.53V$

Hence, the standard electrode potential of the cell is 4.53 V.

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3 years ago