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jeka57 [31]
2 years ago
6

Find the mass of sodium required to reduce 6.58 L of hydrogen gas at 32°C and 895 mm, when sodium reacts with hydrochloric acid.

(Hint: you first need to write a balanced chemical equation.)

Chemistry
1 answer:
Alex2 years ago
3 0

Answer:

Mass = 14.72 g

Explanation:

Given data:

Volume of hydrogen = 6.58 L

Temperature of gas = 32°C (32+273 = 305 k)

Pressure of gas = 895 mmHg (895/760 = 1.2 atm)

Mass of sodium required = ?

Solution:

Chemical equation:

2HCl + 2Na     →      2NaCl + H₂

Number of moles of hydrogen:

PV = nRT

1.2 atm × 6.58 L = n× 0.0821 atm.L/mol.K×305 K

7.9 atm.L =  n×  25.0  atm.L/mol

n = 7.9 atm.L / 25.0  atm.L/mol

n = 0.32 mol

Now we will compare the moles of hydrogen with sodium.

             H₂           :        Na

              1              :        2

            0.32          :     2/1×0.32 = 0.64 mol

Mass of sodium:

Mass = number of moles × molar mass

Mass = 0.64 mol × 23 g/mol

Mass = 14.72 g

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2 years ago
what is the molar mass of a gaseous flouride of sulfur containing 70.4% F and having a density of approximately 4.5g/L at 20 deg
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Answer:

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Explanation:

<u>Step 1:</u> Data given

% of F = 70.4 %

Density = 4.5 g/L

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<u>Step 2:</u> Calculate the number of moles

PV = nRT

 ⇒ with P = the pressure = 1.00 atm

⇒ with V = the volume = Assume this is 1L

⇒ with n = the number of moles = TO BE DETERMINED

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

⇒ T = the temperature : 20°C = 293 Kelvin

1 atm*1L= n(0.08206 L-atm/mol-K)*(293 K)

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<u>Step 3</u>: Calculate molar mass

Molar mass = Mass / moles

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Moles = Mass / molar mass

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Moles S = 0.923 moles S

<u>Step 5:</u> Divide by the smallest amount of moles

F = 3.70 / 0.923 = 4

S = 0.923 / 0.923 = 1

The empirical formula is SF4

The molar mass of SF4 = 32.07 + 4*19 = 108.07 g/mol

This means the empirical formula is the same as the molecular formula SF4

The molar mass is 180.2 g/mol

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