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taurus [48]
3 years ago
12

To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled

it with the gas at 2.00 atm and 24.0 ∘C and weighed it again. The difference in mass was 9.5 g . Identify the gas.
Chemistry
2 answers:
PIT_PIT [208]3 years ago
7 0

Answer:

The gas is nitrogen gas N2

Explanation:

Step 1: Data given

Volume of the gas = 4.1L

Pressure = 2.00 atm

Temperature = 24.0 °C

Mass = 9.5 grams

Step 2: Calculate moles of gas

p*V = n*R*T

n = (p*V)/(R*T)

⇒ with p = the pressure of the diatomic gas = 2.00 atm

⇒ with V = the volume of the diatomic gas = 4.1L

⇒ with n = the moles of the diatomic gas = TO BE DETERMINED

⇒ with R = the gas constant = 0.08206 L*atm/mol *K

⇒ with T = the temperature = 24.0 °C = 297 K

n = (2.00*4.1)/(0.08206*297)

n = 0.336 moles

Step 3: Calculate molar mass

Molar mass = mass / moles

Molar mass = 9.5 grams / 0.336 moles

Molar mass = 28 g/mol = X2

X has a molar mass of 14 g/mol

The gas is nitrogen gas N2

kirza4 [7]3 years ago
6 0

Answer:

Nitrogen, N_2\\

Explanation:

Hello,

This is a clear example of what the ideal gas equation is used for, thus, from its mathematical definition:

PV=nRT

One can spell it out in terms of mass and molar mass:

PV=\frac{m}{M}RT

Now, solving for the molecular mass, M:

M=\frac{mRT}{PV} =\frac{9.5g*0.082\frac{atm*L}{mol*K}*297.15K}{2.00atm*4.1L}\\ M=28.23g/mol

Now, by taking into account that the gas is diatomic, the matching gas turns out to be nitrogen.

Best regards.

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two atoms

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To answer this question, you will need to write the balanced equation and set up a BCA table. Using appropriate rounding rules,
Elenna [48]

Water decomposes when electrolyzed to produce hydrogen and oxygen gas. If 2.5 grams of water were decomposed 1.04 grams of oxygen will be formed.

BCA table:

2H_{2}O ⇒ H_{2} + O_{2}

B  0.13        0 + 0

C  -0.13      0.065 + 0.065

A  0             0.065

Explanation:

Balanced equation for water decomposition into hydrogen and oxygen gases

   2H_{2}O ⇒ H_{2} + O_{2}

B  0.13        0 + 0

C  -0.13      0.065 + 0.065

A  0             0.065

Number of moles of water = \frac{mass}{atomic mass of 1 mole}

mass = 2.5 grams

atomic mass= 18 grams

number of moles can be known by putting the values in the formula,

n = \frac{2.5}{18}

  = 0.13 moles

2 moles of water gives one mole of oxygen on decomposition

so, 0.13 moles of water will give x moles of oxygen on decompsition

\frac{1}{2} = \frac{x}{0.13}

x = 0.065 moles of oxygen will be formed.

moles to gram will be calculated as

mass =number of moles x atomic mass

        = 0.065 x 16

         = 1.04 grams of oxygen.

7 0
3 years ago
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