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Vlad1618 [11]
2 years ago
14

What is the mass of silver chloride.required to plate 295mg.of pure.silver

Chemistry
1 answer:
vekshin12 years ago
3 0


17 hope its correct pls rate 5 star


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At a certain temperature the vapor pressure of pure thiophene is measured to be . Suppose a solution is prepared by mixing of th
Lesechka [4]

Answer:

0.35 atm

Explanation:

It seems the question is incomplete. But an internet search shows me these values for the question:

" At a certain temperature the vapor pressure of pure thiophene (C₄H₄S) is measured to be 0.60 atm. Suppose a solution is prepared by mixing 137. g of thiophene and 111. g of heptane (C₇H₁₆). Calculate the partial pressure of thiophene vapor above this solution. Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution is ideal."

Keep in mind that if the values in your question are different, your answer will be different too. <em>However the methodology will remain the same.</em>

First we <u>calculate the moles of thiophene and heptane</u>, using their molar mass:

  • 137 g thiophene ÷ 84.14 g/mol = 1.63 moles thiophene
  • 111 g heptane ÷ 100 g/mol = 1.11 moles heptane

Total number of moles = 1.63 + 1.11 = 2.74 moles

The<u> mole fraction of thiophene</u> is:

  • 1.63 / 2.74 = 0.59

Finally, the <u>partial pressure of thiophene vapor is</u>:

Partial pressure = Mole Fraction * Vapor pressure of Pure Thiophene

  • Partial Pressure = 0.59 * 0.60 atm
  • Pp = 0.35 atm

3 0
3 years ago
Mg(OH)2 + 2 HBr à MgBr2 + 2 H2O
AnnyKZ [126]

Explanation:

The balanced equation of the reaction is given as;

Mg(OH)2 (s) + 2 HBr (aq) → MgBr2 (aq) + 2 H2O (l)

1. How many grams of MgBr2 will be produced from 18.3 grams of HBr?

From the reaction;

2 mol of HBr produces 1 mol of  MgBr2

Converting to masses using;

Mass = Number of moles * Molar mass

Molar mass of HBr = 80.91 g/mol

Molar mass of MgBr2 = 184.113 g/mol

This means;

(2 * 80.91 = 161.82g) of HBr produces (1 * 184.113 = 184.113g) MgBr2

18.3g would produce x

161.82 = 184.113

18.3 = x

x = (184.113 * 18.3 ) / 161.82 = 20.8 g

2. How many moles of H2O will be produced from 18.3 grams of HBr?

Converting the mass to mol;

Number of moles = Mass / Molar mass = 18.3 / 80.91 = 0.226 mol

From the reaction;

2 mol of HBr produces 2 mol of H2O

0.226 mol would produce x

2 =2

0.226 = x

x = 0.226 * 2 / 2 = 0.226 mol

3. How many grams of Mg(OH)2 are needed to completely react with 18.3 grams of HBr?

From the reaction;

2 mol of HBr reacts with 1 mol of Mg(OH)2

18.3g of HBr =  0.226 mol

2 = 1

0.226 = x

x = 0.226 * 1 /2

x = 0.113 mol

5 0
3 years ago
When excess dilute hydrochloric acid was added to sodium sulphite 960 of sulphuric (iv) oxide was produced. calculate the mass o
irakobra [83]

The mass of sodium sulfite that was used will be 1,890 grams.

<h3>Stoichiometric problems</h3>

First, the equation of the reaction:

NaSO_3 + 2HCl --- > NaCl_2 + H_2O + SO_2

The mole ratio of SO2 produced and sodium sulfite that reacted is 1:1.

Mole of 960 grams SO2 = 960/64 = 15 moles

Equivalent mole of sodium sulfite that reacted = 15 moles

Mass of 15 moles sodium sulfite = 15 x 126 = 1,890 grams

More on stoichiometric problems can be found here: brainly.com/question/14465605

#SPJ1

3 0
1 year ago
PLEASE ANSWER ASAP I WILL GIVE BRAINLIEST!!
anzhelika [568]
It’s lower, hope this helps with your issue and helps solve your problem, no problem
5 0
3 years ago
Read 2 more answers
How many molecules of H2O are there in 1.0 g of H2O?
NISA [10]
Molar mass H₂O = 18.0 g/mol

number of moles :

1.0 / 18.0 => 0.055 moles

1 mole -------------- 6.02 x 10²³ molecules
0.055 moles --------  ? molecules

molecules = 0.055 x ( 6.02 x 10²³) / 1

molecules = 3.311x10²² / 1

= 3.311 x 10²² molecules

hope this helps!
8 0
2 years ago
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