From the list provided, choose the reason that

Give the products of the reaction of butanal, with: (a) sodium borohydride, in methanol (b) hydrogen cyanide, with catalytic cya

miss Akunina [59]

Answer:

Answers are given below

Explanation:

(a) Aldehyde groups are reduced by sodium borohydride in methanol to give alcohol.

So, butanal produces butanol on reaction with sodium borohydride in methanol.

(b) Aldehyde forms cyanohydrin when they are treated with HCN with catalytic cyanide.

(c) Aldehydes are oxidized by potassium dichromate in dil. sulphuric acid to produce carboxylic acid.

(d) Aldehyde produces acetal with methanol and a trace amount of acid catalyst.

(e) Aldehyde gives condensation reaction with $CH_{3}CH_{2}NH_{2}$ to produce imine.

Structures of products for the given reaction has been shown below.

4 0

3 years ago

What is the relationship between atoms and mass?

castortr0y [4]

Answer:

Explanation:

A property closely related to an atom's mass number is its atomic mass. The atomic mass of a single atom is simply its total mass and is typically expressed in atomic mass units or amu.

6 0

3 years ago

I need help answering this question

aleksandrvk [35]

Answer:

it is D

Explanation:

6 0

3 years ago

Read 2 more answers

A Chemist measured 184 mL using a graduated cylinder. Based on her experience, the volume did not seem to be correct. This volum

salantis [7]

Answer:

Percent error = 20%

Explanation:

The percent error is calculated using the following equation:

Percent error = |(approximate value - exact value)| / (exact value) x 100%

In this problem, the approximate value was 184 mL and the exact value was 230.0 mL

Percent error = |(184 mL - 230.0 mL)| / (230.0 mL) x 100% = 20%

8 0

3 years ago

A 12.0 g sample of a metal is heated to 90.0 ◦C. It is then dropped into 25.0 g of water. The temperature of the water rises fro

deff fn [24]

Answer:

The specific heat of the metal is 0.34 J/g°C

Explanation:

Step 1: Data given

Mass of the metal = 12.0 grams

Mass of the water = 25.0 grams

Initial temperature of the metal = 90.0 °C

Initial temperature of the water = 22.5 °C

Final temperature = 25 °C

Specific heat of water = 4.184 J/g°C

Step 2: Calculate the specific heat of the metal

Qlost = Qgained

Q = m*c*ΔT

Qmetal = -Qwater

m(metal) *c(metal)* ΔT(metal) = -m(water) * c(water) *ΔT(water)

⇒ with mass of metal = 12.0 grams

⇒ with c(metal) = TO BE DETERMINED

⇒ with ΔT(metal) = T2 - T1 = 25.0°C - 90.0 °C = -65.0 °C

⇒ with mass of water = 25.0 grams

⇒ with c(water) = 4.184 J/g°C

⇒ with ΔT(water) = T2 - T1 = 25.0 - 22.5 °C = 2.5 °C

12.0 * c(metal) * -65.0 °C = -25.0g * 4.184 J/g°C * 2.5°C

-780.0 * c(metal) = -2615 ( 2.6*10^3 with sig figs)

c(metal) = 0.335 (=0.34 with sig figs)

The specific heat of the metal is 0.34 J/g°C

3 0

3 years ago