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Lisa [10]
3 years ago
8

Rust is formed by the interaction of iron and oxygen. When rust formed on an iron nail with a mass of 100 g, the mass of the rus

ted nail was 143g. What mass of oxygen gas most likely reacted with the iron nail? A) 43g B) 50g C) 100g D) 243g
Chemistry
1 answer:
DanielleElmas [232]3 years ago
6 0

Answer: The correct option is A.

Explanation: Moles of Iron nail can be calculated by using the formula:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}       ...(1)

Given mass of iron nail = 100 g

Molar mass of iron = 56 g/mol

\text{Number of moles}=\frac{100g}{56g/mol}

Number of moles of iron nail = 1.79 moles

The chemical equation for the formation of rust if given by:

4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)

By Stoichiometry of the reaction,

4 moles of iron reacts with 3 moles of oxygen gas to produce 2 moles of rust.

So, 1.79 moles of iron will react with = \frac{3}{4}\times 1.79 = 1.3425 moles of oxygen gas.

For oxygen gas,

Molar mass = 32 g/mol

Mass of oxygen can be calculated by using equation 1, we get

1.3425mol=\frac{\text{Given mass}}{32g/mol}

Mass of oxygen gas = 43 grams

Hence, the correct option is a.

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A solution contains 45 grams of nitrogen gas and 40 grams of argon. What is the mole fraction of argon in this solution?
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 <span>0.38 

You first calculate the total moles by dividing the grams by molecular weight: 
45 g N2 / 28.02 g/mol = 1.6 mol N2 
40 g Ar / 39.95 g/mol = 1.0 mol 

Then you divide the moles of Ar by the total number of moles: 
1.0 / (1.6 + 1.0) = 0.38 mol fraction</span>
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What is the charge on a hypothetical ion with 85 protons and 83 electrons?
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7 0
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Empirical formula of a compound is CH3. If the molar mass of the
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7 0
3 years ago
Which metal will spontaneously react with Zn2+(aq), but will not spontaneously react with Mg2+(aq)?
DerKrebs [107]
Correct Answer: option <span>(1) Mn(s)

Reason: 
The </span><span>spontaneity of electrochemical cell, depends on the it's Eo value. Electrochemical cells with positve Eo are spontanous and vice-versa.
</span>
In present case, the  Eo of half-cell of interest are as follows:
Eo Zn2+/Zn = <span>-0.763v
</span>Eo Mg2+/Mg = 2.37v
Eo Mn2+/Mn = -1.18v

Therefore, Eo cell (with Zn as one of the half-cell) =  Eo Zn2+/Zn - Eo Mn2+/Mn
                                                                                =  -0.763 - (-1.18)
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On other hand, Eo cell (with Mg as one of the half-cell) =  Eo Mg2+/Zn - Eo Mn2+/Mn
                                                                                =  -2.37 - (-1.18)
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Thus, Mn(s) <span>metal will spontaneously react with Zn2+(aq), but will not spontaneously react with Mg2+(aq)</span>
8 0
3 years ago
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