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vladimir1956 [14]
3 years ago
5

You have a gas at 453 mm Hg with a volume of 700 mL and a temperature of 25 °C, what will the temperature of the gas be, if you

change the pressure to 278 mm Hg and a volume of 1200 mL?
Chemistry
1 answer:
jonny [76]3 years ago
7 0
The  temperature  of  a  the gas    is  calculated using   combined  gas  law  formula that is  P1V1/T1  = P2V2/T2
P1  =  453mmhg
V1=  700ml
T1  = 25  +  273  =  298k
P2 = 278 mmhg
V2 = 1200ml
T2=  ?

T2  is therefore  = T1 P2V2/p1V1
=  298   x278   x1200/  453  x  700  =  313.5 K
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A chemist must dilute 61.9 mL of 548. nM aqueous sodium carbonate (Na2CO3) solution until the concentration falls to 484. nM . H
maw [93]

Answer:

The final volume will be "70.08 mL".

Explanation:

The given values are:

Molar mass,

M1 = 548 nM

or,

     = 5.48\times 10^{-7} \ M

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or,

      = 4.84\times 10^{-7} \ M  

Volume,

V1 = 61.9 mL

V1 = ?

By using the expression, we get

⇒ M1\times V1=M2\times V2

or,

⇒            V2=\frac{M1\times V1}{M2}

By substituting the values, we get

                    =\frac{5.48\times 10^{-7}\times 61.9}{4.84\times 10^{-7}}

                    =\frac{339.212}{4.84}

                    =70.08 \ mL

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3 years ago
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Answer:

The element argon is in column 8A and is a noble gas. Nobles gases are completely stable because their outershell is filled with all eight electrons.  Argon has eight valence electrons.

4 0
2 years ago
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The answer is:Matter
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Answer:

B

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