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Monica [59]
3 years ago
12

Four gases were combined in a gas cylinder with these partial pressures: 3.5 atm N2, 2.8 atm O2, 0.25 atm Ar, and 0.15 atm He.

Chemistry
2 answers:
antiseptic1488 [7]3 years ago
7 0

Answer:

P(total) =  6.7 atm

Explanation:

Given data:

Partial pressure of N₂ = 3.5 atm

Partial pressure of O₂ = 2.8 atm

Partial pressure of Ar = 0.25 atm

Partial pressure of He = 0.15 atm

Total pressure = ?

Solution:

According to the Dalton law of partial pressure,

"The total pressure inside the gas cylinder having mixture of gases is equal to the sum of partial pressures of individual gas present in it"

Mathematical expression:

P(total) = P₁ + P₂ + P₃ + .........Pₙ

Now we will determine the total pressure of given gases.

P(total) = P₁ + P₂ + P₃ + P₄

P(total) =P(N₂) + P(O₂) + P(Ar) + P(He)

P(total) = 3.5 atm + 2.8 atm + 0.25 atm + 0.15 atm

P(total) =  6.7 atm

sp2606 [1]3 years ago
5 0

Answer:

6.7 atm

Explanation:

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3 years ago
2. What ions are present in what ratio in a solution of aqueous calcium chloride?
Alenkasestr [34]

Answer:

\mathrm{Ca}^{2+} \text { and } \mathrm{Cl} \text { - ions are present in } 1: 2 \text { ratio in a solution of aqueous calcium chloride. }

Explanation:

Here in Calcium Chloride ionic bond is present in between calcium and chlorine atoms. As we know according to Octet rule calcium have two excess atoms and for matching nearest noble gas electronic configuration. It donate two electrons to gain more stability and form \mathrm{Ca}^{2+}, while chlorine is deficient from one electron to meet nearest noble gas electronic configuration therefore two chlorine atoms accept excess electron from calcium individually and form two\mathrm{Cl}^{-} ions.

\text { Equation is as follows: } \mathrm{Ca}^{2+}+2 \mathrm{Cl}^{-} \rightarrow \mathrm{CaCl}_{2}

Hence aqueous solution of calcium chloride breaks the ionic bond pairing in one \mathrm{Ca}^{2+}and two\mathrm{Cl}^{-}ions: \mathrm{CaCl}_{2} \longrightarrow \mathrm{H}_{2} \mathrm{O} \quad \mathrm{Ca}^{2+}(\mathrm{ag})+2 \mathrm{Cl}(\mathrm{ag})

5 0
3 years ago
What is the maximum number of moles of NaCl that can be produced from the reaction of 5.6 mol Na and 4.7 mol CI2?
RideAnS [48]

Answer:

Explanation:

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8 0
2 years ago
How much mass of sodium chloride ( ) should be dissolved in water to make 1.5 L of 0.75 M aqueous solution? The molar mass of is
iogann1982 [59]

Answer:

Mass = 65.8 g

Explanation:

Given data:

Mass of sodium chloride = ?

Volume of solution = 1.5 L

Molarity of solution = 0.75 M

Solution:

Number of moles of sodium chloride:

Molarity = number of moles / volume in L

By putting values,

0.75 M = number of moles = 1.5 L

Number of moles = 0.75 M × 1.5 L

Number of moles = 1.125 mol

Mass of sodium chloride:

Mass = number of moles × molar mass

Mass = 1.125 mol × 58.5 g/mol

Mass = 65.8 g

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2 years ago
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Answer:

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Explanation:

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