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balu736 [363]
3 years ago
6

A 1.20-L container contains 1.10 g of an unknown gas at STP. What is the molecular weight of the unknown gas?

Chemistry
1 answer:
SOVA2 [1]3 years ago
8 0

Answer:

M = 20.5 g/mol

Explanation:

Given data:

Volume of gas = 1.20 L

Mass of gas = 1.10 g

Temperature and pressure = standard

Solution:

First of all we will calculate the density.

Formula:

d = mass/ volume

d = 1.10 g/ 1.20 L

d = 0.92 g/L

Now we will calculate the molar  mass.

d = PM/RT

0.92 g/L = 1 atm × M / 0.0821 atm.L/mol.K ×273.15 K

M =  0.92 g/L × 0.0821 atm.L/mol.K ×273.15 K /  1 atm

M = 20.5 g/mol

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3 years ago
What is the ph of a 0.006 m koh solution? 1. 11.78 2. 7.00 3. 2.22 4. 8.88 5. 5.12?
Stels [109]
The concentration of OH⁻ is first converted to pOH bu using followinf formula,

                                           pOH  =  -log [OH⁻]
Putting value,
                                           pOH  =  -log (0.006)

                                           pOH  =  2.221
As we know,
                                   pH + pOH  =  14
Solving for pH,
                                   pH  =  14 - pOH
Putting value of pOH,
                                   pH  =  14 - 2.221

                                   pH  =  11.779
Result:
           Option-1
is the correct answer.
4 0
3 years ago
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