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ipn [44]
3 years ago
7

What mass of sodium hydroxide will completely neutralize 2.5 mol of sulfuric acid?

Chemistry
1 answer:
VMariaS [17]3 years ago
7 0

Given :

2.5 mole of Sulfuric acid ( H_2SO_4 ) .

To Find :

Mass of sodium hydroxide will completely neutralize 2.5 mol of sulfuric acid

Solution :

Let us assume volume of water be 1 L .

Now , we know , to neutralize 1 mole of sulfuric acid we need 2 moles of NaOH .

So , for 2.5 mole sulfuric acid required 5 mole of NaOH .

Moles of NaOH ,

n=M\times Volume \\\\n=5\times 1=5\ moles  

Molecular mass of NaOH , M.M = 58.44 g/mol .

Mass of 5 moles of NaOH :

m=5\times 58.44\ g\\\\m=292.2\ g

Hence , this is the required solution .

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C10H22 > C8H18+C2H4 if only ethane can be sold what is the atom econmy of this process
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Answer:

The atom economy of ethane in this process is 19.72 %.

What is atom economy?

The conversion efficiency of a chemical reaction in terms of all the atoms involved and the desired products produced is known as atom economy (atom efficiency/percentage).

Explanation:

C₁₀H₂₂ → C₈H₁₈ + C₂H₄

Molecular weight of C₁₀H₂₂ = 142.28

Molecular weight of C₈H₁₈ = 114.228
Molecular weight of C₂H₄ = 28.053

% Atom economy =     \frac {Molecular weight of C2H4} {Molecular weight of C10H22}

                             = \frac{28.053}{142.28}*100

                             = 19.716 %

                             ≈ 19.72 %


To know more about atom economy, click on the link

brainly.com/question/17159753

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For the first order process: AB The half-life of A is 62.1 seconds. If a sample of A initially has 250.0 g, what mass (in g) of
Molodets [167]

<u>Answer:</u> The mass of sample A after given time is 99.05 g.

<u>Explanation:</u>

All the radioactive reactions follows first order kinetics.

The equation used to calculate half life for first order kinetics:

t_{1/2}=\frac{0.693}{k}

We are given:

t_{1/2}=62.1s

Putting values in above equation, we get:

k=\frac{0.693}{62.1}=0.011s^{-1}

Rate law expression for first order kinetics is given by the equation:

k=\frac{2.303}{t}\log\frac{[A_o]}{[A]}

where,

k = rate constant = 0.011s^{-1}

t = time taken for decay process = 84.2 s

[A_o] = initial amount of the reactant = 250 g

[A] = amount left after decay process =  ?

Putting values in above equation, we get:

0.011s^{-1}=\frac{2.303}{84.2s}\log\frac{250}{[A]}

[A]=99.05g

Hence, the mass of sample A after given time is 99.05 g.

5 0
2 years ago
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