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Rufina [12.5K]
2 years ago
13

What are the masses of the four different brcl molecules?

Chemistry
1 answer:
tatyana61 [14]2 years ago
7 0

Through mass spectrometry, we can define 4 different isotopes of the BrCl molecule:

⁸¹Br³⁷Cl, ⁸¹Br³⁵Cl, ⁷⁹Br³⁷Cl, ⁷⁹Br³⁵Cl  

Masses of the different individual isotopes:

³⁷Cl=36.966

³⁵Cl=34.968

⁸¹Br=80.916

⁷⁹Br=78.918

Masses of 4 different isotopes of the BrCl molecule:

⁸¹Br³⁷Cl=80.916+36.966=117.882

⁸¹Br³⁵Cl=80.916+34.968=115.884

⁷⁹Br³⁷Cl=78.918+36.966=115.884

⁷⁹Br³⁵Cl=78.918+34.968=113.886

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<u>Answer:</u>

<em>Latest take an example to understand how </em><em>balancing of chemical reaction</em><em> is done that is assuming the reaction between iron as well as </em><em>oxygen which reacts to form rust.</em>

<u>Explanation:</u>

For this we would simply right the reactant and product that is expected. Then we would see the number of molecules of each element present on either side.

If in the reaction the element’s molecules are the same on both sides then the reaction would be correct and if not then we have to apply trial and error method to balance the equation such that the number of molecules of each element is equal on both sides of the reaction.

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3 years ago
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PLEASE HELP ME 20 POINTS!!!!!
julsineya [31]

Answer:

Theoretical yield of the reaction is 121·38 g

The excess reactant is hydrogen

The limiting reactant is nitrogen

Explanation:

By assuming that the reaction between nitrogen and hydrogen taking place in presence of catalyst because at normal conditions the reaction between them will not occur

Number of moles of nitrogen taken are 100÷28 ≈ 3.57

Number of moles of hydrogen taken are 100÷2 = 50

Actually the reaction between nitrogen and hydrogen takes place according to the following equation

<h3>Nx_{2} + 3Hx_{2}  → 2NHx_{3}</h3>

So from the equation for 1  mole of nitrogen and 3 moles of hydrogen we get 2 moles of ammonia

Here in the problem we have approximately 3·57 moles of nitrogen so we require 3×3·57 moles of hydrogen

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But we have 50 moles of hydrogen

∴ Excess reagent is hydrogen and limiting reagent is nitrogen

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Weight of ammonia is 17 g

∴ Amount of ammonia produced is 17×7·14 = 121·38 g

∴ Theoretical yield of the reaction is 121·38 g

5 0
3 years ago
When the temperature in a room increases from 25°C to 33°C, changes from a solid to a liquid.
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Answer:

true

Explanation:

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Carbon dioxide (CO2) is a gas at room temperature and pressure. However, carbon dioxide can be put under pressure to become a "s
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Answer:

The mass of this 25 mL supercritical CO2 sample has a mass of 11.7g

Explanation:

Step 1: Given data

The supercritical CO2 has a density of 0.469 g/cm³ (or 0.469 g/mL)

The sample hasa volume of 25.0 mL

Step 2: Calculating mass of the sample

The density is the mass per amount of volume

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