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lubasha [3.4K]
3 years ago
13

Calculate the empirical formula for a compound containing 67.6% Hg 10.8% S 21.6% O

Chemistry
1 answer:
pashok25 [27]3 years ago
3 0

Answer:

HgSO₄

Explanation:

% => g => moles => ratio => reduce => empirical ratio

%Hg = 67.6% => 67.6g/201g/mol = 0.34mol

%S    = 10.8% => 10.8g/32g/mol = 0.34mol

%O   = 21.6% => 21.6g/16g/mol = 1.35mol

Hg:S:O => 0.34:0.34:1.35

Reduce to whole number ratio by dividing by the smaller mole value...

Hg:S:O => 0.34/.34:0.34/.34:1.35/.34 => Empirical Ratio = 1:1:4

∴ Empirical Formula is HgSO₄

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Lead(II) nitrate and ammonium iodide react to form lead(II) iodide and ammonium nitrate according to the reaction Pb(NO3)2(aq)+2
Setler79 [48]

Answer:

a) volume of ammonium iodide required =349 mL

b) the moles of lead iodide formed = 0.0436 mol

Explanation:

The reaction is:

Pb(NO_{3})_{2}+2NH_{4}I -->PbI_{2}+2NH_{4}NO_{3}

It shows that one mole of lead nitrate will react with two moles of ammonium iodide to give one mole of lead iodide.

Let us calculate the moles of lead nitrate taken in the solution.

Moles=molarityX volume (L)

Moles of lead nitrate = 0.360 X 0.121 =0.0436 mol

the moles of ammonium iodide required = 2 X0.0436 = 0.0872 mol

The volume of ammonium iodide required will be:

volume=\frac{moles}{molarity}=\frac{0.0872}{0.250}=0.349L=349mL

the moles of lead iodide formed = moles of lead nitrate taken = 0.0436 mol

7 0
3 years ago
Webb has calculated the percent composition of a compound. How can he check his result?
fenix001 [56]
Webb has calculated the percent composition of a compound. He can check his result by adding them to see if they equal up to 100. Why? Well, percent composition tells the quantity of elements with 100 as a base of total amount. This means that it will have to add to 100 to check the result. You would add up all of the values of percent composition of elements to see if they equal 100, and if they do, the results are accurate.

Your final answer: Webb can check his result by seeing if they add up to 100, considering that is the base total quantity.
7 0
2 years ago
Calculate the number of moles equivalent to 12.7 gram of iodine molecule ​
Alexus [3.1K]

\LARGE{ \boxed{ \purple{ \rm{Answer}}}}

☃️ Chemical formulae ➝ \sf{I_2}

How to find?

For solving this question, We need to know how to find moles of solution or any substance if a certain weight is given.

\boxed{ \sf{No. \: of \: moles =  \frac{Given \: weight}{Molecular \: weight} }}

Solution:

❍ Molecular weight of \sf{I_2}

= 2 × 126.90

= 253.80

= 254 (approx.)

❍ Given weight: 12.7

Then, no. of moles,

⇛ No. of moles = 12.7 / 254

⇛ No. of moles = 0.05 moles

⚘ No. of moles of Iodine molecule in the given weight = <u>0.05</u><u> </u><u>moles </u>

<u>━━━━━━━━━━━━━━━━━━━━</u>

6 0
3 years ago
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What are the benefits of a model to demonstrate the atomic theory?
Norma-Jean [14]

Answer:

Atomic models are important because, they help us visualize the interior of atoms and molecules, and thereby predicting properties of matter.

Explanation:

We study the various atomic models in our course of study because, it is important for us to know, how did people come to the present concept of an atom. How did physics evolve from classical to quantum physics.

All these are important for us to know and thus, knowledge about various atomic models, their discoveries and drawbacks and finally improvements based on scientific evidence present at that time is important for us to understand the underlying theory very well.

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How many moles in 32.7 grams of water vapor?
mestny [16]
To find moles from grams divide the number of moles by the molar mass...

32.7g/18.01 which is 1.82 using significant figure rules
4 0
3 years ago
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