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LUCKY_DIMON [66]
1 year ago
15

The reaction na 3po 4( aq) 3 agno3( aq) → ag 3po 4( s) 3 nano 3( aq) is best classified as a(n):_____.

Chemistry
1 answer:
Ugo [173]1 year ago
6 0

The reaction  Na_{3} PO_{4} ( aq) +3AgNO_{3} (aq) → Ag_{3} PO_{4} ( aq) +3NaNO_{3} (aq) is best classified as double displacement reaction.

Those reaction in which two compounds react by exchanges of ions to form two new compounds is called  double displacement reaction. The easiest way to identify double displacement reactions is to check to see whether the cations exchanged anions with each other  or not . Always balanced chemical equation is used to determine.

There are three types of double displacement reaction which is given as,

  1. Precipitation
  2. Neutralization
  3. Gas formation

The real world example of double displacement reaction is combining vinegar and baking soda to create homemade volcano.

learn more about double displacement reaction

brainly.com/question/13870042?

#SPJ4

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The partial pressure of CO2 gas in a bottle of carbonated water is 4.60 atm at 25 ºC. How much CO2 gas (in g) will be released f
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If the partial pressure of CO₂ in a bottle of carbonated water decreases from 4.60 atm to 1.28 atm, the mass of CO₂ released is 0.265 g.

The partial pressure of CO₂ gas in a bottle of carbonated water is 4.60 atm at 25 ºC. We can calculate the concentration of CO₂ using Henry's law.

C = k \times P = \frac{1.65 \times 10^{-3} M }{atm}  \times 4.60 atm = 7.59 \times 10^{-3} M

We can calculate the mass of CO₂ in 1.1 L considering its molar mass is 44.01 g/mol.

\frac{7.59 \times 10^{-3} mol}{L} \times  1.1 L \times \frac{44.01 g}{mol}  = 0.367 g

Now, we will repeat the same procedure for a partial pressure of 1.28 atm.

C = k \times P = \frac{1.65 \times 10^{-3} M }{atm}  \times 1.28 atm = 2.11 \times 10^{-3} M

\frac{2.11 \times 10^{-3} mol}{L} \times  1.1 L \times \frac{44.01 g}{mol}  = 0.102 g

The mass of CO₂ released will be equal to the difference in the masses at the different pressures.

m = 0.367 g - 0.102 g = 0.265 g

If the partial pressure of CO₂ in a bottle of carbonated water decreases from 4.60 atm to 1.28 atm, the mass of CO₂ released is 0.265 g.

Learn more: brainly.com/question/18987224

<em>The partial pressure of CO₂ gas in a bottle of carbonated water is 4.60 atm at 25 ºC. How much CO₂ gas (in g) will be released from 1.1 L of the carbonated water when the partial pressure of CO2 is lowered to 1.28 atm? At 25 ºC, the Henry’s law constant for CO₂ dissolved in water is 1.65 x 10⁻³ M/atm, and the density of water is 1.0 g/cm³.</em>

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