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zlopas [31]
3 years ago
6

Calculate the extinction coefficient where the concentration is in mg/ml and the path length is 1 cm. What dilutions of the stoc

k are each of the prepared solutions (i.e., 1/x)?
The molecular weight of A is 290 g/mole.
Re-calculate the extinction coefficient with the concentration in mM. Note that the newly calculated extinction coefficient will contain an mM-1 term.

Chemistry
1 answer:
Airida [17]3 years ago
4 0

Complete Question

The complete question is show on the first uploaded image

Answer:

This is shown on the second,third , fourth and fifth image

Explanation:

This is shown on the second,third , fourth and fifth image

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Draw the product of the reaction between CH3CH=CHCH3 and H2 under a platinum catalyst.
Pani-rosa [81]

Answer:

CH₃CH₂-CH₂CH₃

Explanation:

When an alkene, R-CH=CH-R reacts with H₂ in a Pt catalyst, the analogue alkane, R-CH₂-CH₂-R, is produced (Hydrogenation of alkenes via Pt/Pd catalyst)

Thus, the reaction of CH₃CH=CHCH₃ with H₂ under a platinum catalyst produce:

<h3>CH₃CH₂-CH₂CH₃</h3>

The analogue alkane

4 0
3 years ago
An analytical chemist weighs out 0.055g of an unknown triprotic acid into a 250mL volumetric flask and dilutes to the mark with
Katarina [22]

Answer:

Mass of the unknown acid is 4.0g

Explanation:

The determine the molar mass of the unknown acid, the steps below can be followed

Firstly, determine the concentration of the acid, the formula below can be used;

ConcA × Va/ConcB × Vb = Na/Nb

Where ConcA is the concentration of the unknown acid

ConcB is the concentration of the NaOH base

Va is the volume of acid and Vb is the volume of base

Since, the titration was said to have reached an equivalent point, it means the number of moles of the acid (Na) was equal to the number of moles of the base (Nb) and thus both will be assumed to be 1

Thus

ConcA × 250/0.13 × 6.6 = 1/1

ConcA = 0.13 × 6.6/250

ConcA = 0.003432M

Then, determine the actual number of moles (n) of the unknown acid used,

ConcA = no of moles of acid/volume of acid (in dm³ or L)

To convert mL to L, we divide by 1000

Hence, 250ml = 0.25L

0.003432 = n/0.25

n = 0.003432 × 0.25

n = 0.01373 moles

To determine the molar mass;

n = mass/molar mass

The mass was given in the question to be 0.055g

Thus

0.01373 = 0.055/molar mass

molar mass = 0.055/0.01373

molar mass = 4.0g

5 0
3 years ago
Determine whether the following statements describe chemical or physical properties: (a) Oxygen gas supports combustion. (b) Fer
sdas [7]

Explanation:

A change that does not cause any change in chemical composition of a substance is known as a physical change.

For example, mass, density, volume etc are all physical changes.

On the other hand, a change that brings change in chemical composition of a substance is known as chemical change.

For example, combustion, toxicity, reactivity etc are all chemical changes.

Hence, following statements are identified as chemical or physical changes as follows.

(a) Oxygen gas supports combustion : Chemical change

(b) Fertilizers help to increase agricultural production : Chemical change

(c) Water boils below 100^{o}C on top of a mountain : Physical change

(d) Lead is denser than aluminum : Physical change

(e) Uranium is a radioactive element : Chemical change

7 0
3 years ago
How is enthalpy used to predict whether a reaction is endothermic or exothermic?
Sever21 [200]
<span>The value of enthalpy of a reaction can be a useful tool in determining the type of reaction it is. If the enthalpy is negative the reaction is exothermic and if the enthalpy is positive the reaction is endothermic. Hope this answers the question. Have a nice day.</span>
4 0
3 years ago
At what temperature (°C) will a 10.00 g sample of neon gas exert a pressure of 96.7 kPa in a
Eva8 [605]

Answer : The temperature of neon gas will be, 221.0 K

Explanation :

To calculate the temperature of neon gas we are using ideal gas equation.

PV=nRT\\\\PV=\frac{w}{M}RT

where,

P = pressure of neon gas = 96.7 kPa = 0.955 atm

Conversion used : (1 atm = 101.3 kPa)

V = volume of neon gas = 9.50 L

T = temperature of neon gas = ?

R = gas constant = 0.0821 L.atm/mole.K

w = mass of neon gas = 10.00 g

M = molar mass of neon gas = 20 g/mole

Now put all the given values in the ideal gas equation, we get:

(0.955atm)\times (9.50L)=\frac{10.00g}{20g/mole}\times (0.0821L.atm/mole.K)\times T

T=221.0K

Therefore, the temperature of neon gas will be, 221.0 K

7 0
3 years ago
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