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kkurt [141]
3 years ago
6

(11) su pilateThe substance which is most suitable for drying ammonia is​

Chemistry
1 answer:
damaskus [11]3 years ago
4 0

Answer:mark as brainliest

Explanation:H2SO4 and anhydrous calcium chloride CaCl2 are not used to dry ammonia because they react with it. The gas is passed through fresh quicklime (solid calcium oxide lumps) to effectively dry it.

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Which postulate of dalton's atomic theory not relevant anymore?explain
VLD [36.1K]

Modern atomic theory is, of course, a little more involved than Dalton's theory but the essence of Dalton's theory remains valid. Today we know that atoms can be destroyed via nuclear reactions but not by chemical reactions. Also, there are different kinds of atoms (differing by their masses) within an element that are known as "isotopes", but isotopes of an element have the same chemical properties.

Many heretofore unexplained chemical phenomena were quickly explained by Dalton with his theory. Dalton's theory quickly became the theoretical foundation in chemistry.

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3 years ago
Help please (chemistry homework)
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What is mechanical advantage?
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Answer:

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3 0
3 years ago
Find the empirical formula of each of the following compounds. Given mass or for each element in a sample of the compound 3,611
KengaRu [80]

Answer:

CaCl₂  

Step-by-step explanation:

The <em>empirical formula</em> is the simplest whole-number ratio of atoms in a compound.

The ratio of atoms is the same as the ratio of moles.

So, our job is to calculate the molar ratio of Ca to Cl.

Data:

Mass of Ca = 3.611 g

Mass of Cl = 6.389 g

Calculations

Step 1. <em>Calculate the moles of each element </em>

Moles of Ca = 3.611 g Ca × (1 mol Ca/(40.08 g Ca)= 0.090 10 mol Ca

Moles of Cl = 6.389 g Cl  

Step 2. <em>Calculate the molar ratio of the elements </em>

Divide each number by the smallest number of moles

Ca:Cl = 0.090 10:0.1802 = 1:2.000

Step 3. Round the molar ratios to the nearest integer

Ca:Cl = 1:2.000 ≈ 1:2


Step 4: <em>Write the empirical formula </em>

EF = CaCl₂

8 0
3 years ago
A gas with a pressure of 820.4 mmHg occupies a
irga5000 [103]

Answer:

V₂ = 1223.2 mL  

Explanation:

Given data:

Pressure of gas = 820.4 mmHg

Initial volume of gas = 900.0 mL

Initial temperature = 25.0°C (25+273=298K)

Final temperature = 132.0°C (132.0 +273 = 405 K)

Final volume = ?

Solution:

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁  

V₂ = 900.0 mL × 405 K / 298 k

V₂ = 364500 mL.K / 298 K

V₂ = 1223.2 mL  

5 0
3 years ago
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