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3 years ago

Name 2 separate problems that occur when a sample for infrared analysis is contaminated with water.

Chemistry

1 answer:

Andreyy893 years ago

7 0

Explanation:

The water molecules gets trapped in the crystal structure to be analysed and will give a peak in the spectra at about 3500 /cm , and there by hindering with the IR spectra of the sample to be analysed .
The second problem with the contamination of the sample with water is , that water makes the potassium bromide disc opaque which will decrease the absorption of the IR by the sample .

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How many liters of a 3 M NaOH stock solution would you need to make 552 mL of a 105 mM NaOH dilution

Ganezh [65]

Answer:

0.01932 L

Explanation:

First we convert 105 mM to M:

105 mM / 1000 = 0.105 M

Next we convert 552 mL to L:

552 mL / 1000 = 0.552 L

Then we use the following equation:

C₁V₁=C₂V₂

Where:

C₁ = 3 M

V₁ = ?

C₂ = 0.105 M

V₂ = 0.552 L

We input the given data:

3 M * V₁ = 0.105 M * 0.552 L

And solve for V₁:

V₁ = 0.01932 L

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3 years ago

what would the percentage of thorium-232 ( parent compound) be in a rock that was dated at 1.8 billion years

vovikov84 [41]

The half-life of Th-232 is 1.405 × 10¹⁰ years

Time elapsed = 2.8 x 10⁹ years

Equation of radioactive decay:

A = A₀ = (1/2)^ t/t₁/₂

Thus, the percentage of thorium-232 in the rock that was dated at 2.8 billions year = 87.1%

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3 years ago

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enyata [817]

Answer:

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Explanation:

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3 years ago

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Hello, So I was wondering if this is correct... Is it?

Sonja [21]

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3 years ago

Read 2 more answers

Cu+2AgNO

baherus [9]

Answer:

Mass of Ag produced = 64.6 g

Note: the question is, how many grams of Ag is produced from 19.0 g of Cu and 125 g of AgNO3

Explanation:

Equation of the reaction:

Cu + 2AgNO3 ---> 2Ag + Cu(NO3)2

From the equation above, 1 mole of Cu reacts with 2 moles of AgNO3 to produce 2 moles of Ag and 1 mole of Cu(NO3)2.

Molar mass of the reactants and products are; Cu = 63.5 g/mol, Ag = 108 g/mol, AgNO3 = 170 g/mol, Cu(NO3)2 = 187.5 g/mol

To determine, the limiting reactant;

63.5 g of Cu reacts with 170 * 2 g of AgNO3,

19 g of Cu will react with (340 * 19)/63.5 g of AgNO3 =101.7 g of AgNO3.

Since there are 125 g of AgNO3 available for reaction, it is in excess and Cu is the limiting reactant.

63.5 g of Cu reacts to produce 108 * 2 g of Ag,

19 g of Cu will react to produce (216 * 19)/63.5 g of Ag = 64.6 g of Ag.

Therefore mass of Ag produced = 64.6g

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3 years ago