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2 years ago

How to convert butanoic acid to propanamide?

1 answer:

8 0

Butanoic acid is converted to propanamide by first converting it to propanoic acid, then ammonium propanoate and then finally propanamide by heating.

<h3>How are carboxylic acids converted to amides?</h3>

Carboxylic acids are converted to amides by converting them into into an ammonium salt which then produces an amide on heating.

The ammonium salt is prepared by adding ammonium carbonate to an excess of the acid. The ammonium salt is then heated to give the amide

Therefore, butanoic acid is converted to propanamide by first converting it to propanoic acid, then ammonium propanoate and then finally propanamide by heating.

In conclusion, carboxylic acids are converted to amides in two steps.

Learn more about carboxylic acids and amides at: brainly.com/question/9616270

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Cecil writes the equation for the reaction of hydrogen and oxygen below.

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Answer:

C) to show that atoms are conserved in chemical reactions

Explanation:

When writing a chemical reaction, we should always consider the Mass Conservation Law, which basically states that; in an isolated system; the total mass should remain constant, this is, the total mass of the reactives should be equal to the total mass of the products

For this case, we should add the apporpiate coefficients in order to be in compliance with this law:

2H₂ + O₂ → 2H₂O

So, we can check the above statement:

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3 years ago

Which of the following is not a possible termination step in the free radical chlorination of methane? Group of answer choices ∙

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Answer: first option is not a termination

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3 years ago

A frictionless piston cylinder device is subjected to 1.013 bar external pressure. The piston mass is 200 kg, it has an area of

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Answer:

a) $T_{2} = 360.955\,K$ , $P_{2} = 138569.171\,Pa\,(1.386\,bar)$ , b) $T_{2} = 347.348\,K$ , $V_{2} = 0.14\,m^{3}$

Explanation:

a) The ideal gas is experimenting an isocoric process and the following relationship is used:

$\frac{T_{1}}{P_{1}} = \frac{T_{2}}{P_{2}}$

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$Q = n\cdot \bar c_{v}\cdot (T_{2}-T_{1})$

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The number of moles of the ideal gas is:

$n = \frac{P_{1}\cdot V_{1}}{R_{u}\cdot T_{1}}$

$n = \frac{\left(101,325\,Pa + \frac{(200\,kg)\cdot (9.807\,\frac{m}{s^{2}} )}{0.15\,m^{2}} \right)\cdot (0.12\,m^{3})}{(8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K} )\cdot (298\,K)}$