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3 years ago

Ch2(c(ch3) 2 iupac name

Chemistry

1 answer:

Slav-nsk [51]3 years ago

5 0

Answer:

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A hot lump of 30.5 g of iron at an initial temperature of 52.7 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to r

slava [35]

Answer:

26.7°C

Explanation:

Using the formula; Q = m × c × ΔT

Where; Q = amount of heat

m = mass

c = specific heat

ΔT = change in temperature

In this question involving iron placed into water, the Qwater = Qiron

For water; m= 50g, c = 4.18 J/g°C, Initial temp= 25°C, final temp=?

For iron; m = 30.5g, c = 0.449J/g°C, Initial temp= 52.7°C, final temp=?

Qwater = -(Qiron)

m × c × ΔT (water) =- {m × c × ΔT (iron)}

50 × 4.18 × (T - 25) = - {30.5 × 0.449 × (T - 52.7)}

209 (T - 25) = - {13.6945 (T - 52.7)}

209T - 5225 = -13.6945T + 721.7

209T + 13.6945T = 5225 + 721.7

222.6945T = 5946.7

T = 5946.7/222.6945

T = 26.7

Hence, the final temperature of water and iron is 26.7°C

8 0

3 years ago

What happens when the kinetic energy of molecules increases so much that electrons are released by the atoms, creating a swirlin

iogann1982 [59]

The answer is d in this case

4 0

3 years ago

Read 2 more answers

What is the density of a liquid if the volume is 25 mL and the mass is 20.0 g?

LenKa [72]

Answers:

Density = 0.8 g/mol.

Given data:

v = 25 ml

m = 20 g

δ = ?

Solution:

Formula for calculating density is given as,

Density = Mass / Volume

putting values

Density = 20.0 g / 25 ml

Density = 0.8 g/mol.

3 0

3 years ago

A current of 5. 68 a is passed through a Fe(NO3)2 solution. How long, in hours, would this current have to be applied to plate o

daser333 [38]

There are 1.2 hr would this current have to be applied to plate out 7. 20 g of iron .

Calculation ,

Given ; Current ( I ) = 5. 68 A

In $Fe(NO_{3} )_{2}$ , the valancy of Fe is +2 .

2 moles of $e^{-}$ are required for the decomposition of 1 mole of Fe .

7. 20 g of Fe in moles = 7. 20 g /55.845 g/mol =0.12 mole

x moles of $e^{-}$ are required for the decomposition of 0.128 mole of Fe .

moles of $e^{-}$ are required = 0.256 moles

Charge on 1 mole of $e^{-}$ = 96500 C

Charge on 0.256 mole of $e^{-}$ = 24704 C

Current ( I )= Q/t

t =Q / I = 24704 C/5. 68 A = 4349 sec = 1.2 hr

Therefore , there are 1.2 hr would this current have to be applied to plate out 7. 20 g of iron .

To learn more about iron

brainly.com/question/18500540

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8 0

1 year ago

A solution contains 22.4 g glucose (C6H12O6 ) dissolved in 0.500 L of water. What is the molality of the solution

Shalnov [3]

Answer:

Molality is 0.25 m

Explanation:

Molality → Moles of solute / kg of solvent

We need the moles of solute → 0.124 moles

22.4 g . 1 mol / 180 g = 0.124 moles

We need the mass of solvent in kg. We determine the mass of solvent with density.

Density = Mass / Volume

Mass = Density . volume → 1 g/mL . 500 mL = 500 g

If we convert the mass in g to kg → 500 g . 1kg / 1000 g = 0.5 kg

In conclussion, molality → 0.124 mol / 0.5 kg = 0.25 m

8 0

3 years ago

Ch2(c(ch3) 2 iupac name​

Ch2(c(ch3) 2 iupac name