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barxatty [35]
3 years ago
10

CH4 + 202 → CO2 + 2H2O How many grams of O2 needed to produce 36 grams of H2O?

Chemistry
1 answer:
Pavel [41]3 years ago
8 0

Answer:

Mass = 64 g

Explanation:

Given data:

Mass of water produced = 36 g

Mass of oxygen needed = ?

Solution:

Chemical equation:

CH₄ + 2O₂       CO₂ + 2H₂O

Number of moles of water produced:

Number of moles = mass/molar mass

Number of moles = 36 g/ 18 g/mol

Number of moles = 2 mol

Now we will compare the moles of water and oxygen.

             H₂O       :          O₂

                2         :           2

Mass of oxygen:

Mass = number of moles × molar mass

Mass =  2 mol × 32 g/mol

Mass = 64 g

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How many solutions are there in the following equation.
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Use the following half-reactions to write three spontaneous reactions, calculate E°cell for each reaction, and rank the oxidizin
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Answer:

See explaination

Explanation:

1)

we know that

half cell with higher reduction potential is cathode

so

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anode :

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so

overall reaction is

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now

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so

EO cell = 1.77 + 0.74

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now

in this case

oxidizing agents are N20 and Cr+3

reducing agents are Cr and N2

higher the reduction potential , stronger the oxidizing agent

lower the reduction potential , stronger the reducing agent

so

oxidzing agents

N20 > Cr+3

reducing agents

Cr > N2

2)

cathode :

Au+ + e- --> Au

anode :

Cr ---> Cr+3 + 3e-

overall reaction

3Au+ + Cr ---> 3Au + Cr+3

Eo cell = 1.69 + 0.74

Eo cell = 2.43

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Au+ > Cr+3

reducing agents :

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3)

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N20 + 2H+ + 2e- ---> N2 + H20

andoe :

Au ---> Au+ + e-

overall

2 Au + N20 + 2H+ --> 2 Au+ + N2 + H20

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reducing agents

Au > N2

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