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3 years ago

One atmosphere (atm) is equal to which of the following?

Chemistry

2 answers:

Blababa [14]3 years ago

8 0

The correct answer is D. 760 mm of mercury

Explanation:

One atmosphere (atm) is a unit used to measure pressure (force applied to an object, gas, substance); this unit represents the regular natural pressure that exists at sea level. Additionally, an atmosphere can be equivalent over other pressure units including pascals as 101325 pascals are equivalent to 1 atm; kilopascals as 101.325 kilopascals are the same that 1 atm and even mercury millimeters (mmHg) as one atmosphere is equal to 760 mmHg. Thus, it can be concluded an atmosphere is equal to "760mm of mercury" because this is the only option in which there is a correct equivalence between the atmosphere unit and other units use to measure pressure.

djverab [1.8K]3 years ago

6 0

I’m pretty sure it’s 760 mmHG (mm of mercury)

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A current is applied to two electrolytic cells in series. In the first, silver is deposited; in the second, a zinc electrode is

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The amount of Ag plated out if 1.2 g of Zn dissolves is 3.959 g .

Given ,

A current is applied to two electrolytic cells in series .

In the first ,silver is deposited and in the second a zinc electrode is consumed .

the reactions involving are ;

Ag+ (aq) + e = Ag

Zn = Zn2+ (aq) +2e

thus the resultant equation is ,

2Ag+ (aq) +Zn = 2Ag + Zn2+

Thus for every mole of Zn dissolves , there is 2 moles of Ag is formed .

65.38 g of Zn contains = 1 moles

1.2 g of Zn contains = 1.2/65.38 =0.01835 moles

for every 1 mole of Zn dissolves there is 2 moles of Ag formed .

Thus the amount of Ag formed in moles =2(O.01835) =0.0367 Moles

1 mole of Ag contains = 107.86g

0.0367 moles of Ag contains = 107.86 (0.0367) =3.959 g of Ag

Hence ,the amount of Ag plated out if 1.2 g of Zn dissolves is 3.959 g .

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1 year ago

You have arrived on a planet where S2, not O2, is the gas used as fuel in combustion reactions. When gaseous propane (C3H8) is b

Debora [2.8K]

Answer:

Mass = 53.45 g

Explanation:

Given data:

Mass of propane = 200 g

Mass of S₂ = 75 g

Theoretical yield /Mass of CS₂ = ?

Solution:

Balanced Chemical equation:

C₃H₈ + 5S₂ → 4H₂S + 3CS₂

Number of moles of propane:

Number of moles = mass / molar mass

Number of moles = 200 g/ 44.1 g/mol

Number of moles = 4.54 mol

Number of moles of S₂:

Number of moles = mass / molar mass

Number of moles = 75 g/ 64.14 g/mol

Number of moles = 1.17 mol

Now we will compare the moles of carbon disulfide with both reactant.

S₂ : CS₂

5 : 3

1.17 : 3/5×1.17 = 0.702

C₃H₈ : CS₂

1 : 3

4.54 : 3×4.54 = 13.62 mol

Number of moles of CS₂ produced by S₂ are less so it will limiting reactant and limit the yield of carbon disulfide.

Theoretical yield of carbon disulfide.

Mass = number of moles ×molar mass

Mass = 0.702 mol × 76.14 g/mol

Mass = 53.45 g

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