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3 years ago

A double-replacement reaction, the ____.

Chemistry

1 answer:

vladimir1956 [14]3 years ago

4 0

Answer:

b. reactants are two ionic compounds.

Explanation:

A double-replacement reaction is different from a single-replacement reaction because a double-replacement reaction is a reaction between two ionic compounds while in a single-replacement reaction one atom replace another atom. In addition, the product formed from a double-replacement reaction often precipitate from the given solution.

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A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.116 M and a total blood volume of 4.7 L .

klemol [59]

Explanation:

Normal moles of $Na^{+}$ = volume × normal concentration

= 4.7 × 0.139 = 0.6533 mol

Moles of $Na^{+}$ in hyponatremia blood = volume × hyponatremia concentration

= 4.7 × 0.116 = 0.5452 mol

Moles of NaCl to be added = moles of extra $Na^{+}$ needed

= 0.6533 mol - 0.5452 mol = 0.1081 mol

Mass of NaCl = moles × molar mass of NaCl

= 0.1081 mol × 58.443

= 6.317g

= 6.32 g (approx)

Thus, we can conclude that mass of sodium chloride would need to be added to the blood is 6.32 g.

3 0

3 years ago

What would a substance that could undergo condensation polymerization most likely have? two double bonds a triple bond two aldeh

blagie [28]

The fourth option on Edgen, "two alcohol functional groups". You're welcome :)

5 0

3 years ago

Read 2 more answers

A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). W

Agata [3.3K]

Answer : The 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

Explanation :

Galvanic cell : It is defined as a device which is used for the conversion of the chemical energy produces in a redox reaction into the electrical energy. It is also known as the voltaic cell or electrochemical cell.

In the galvanic cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.

We are taking the value of standard reduction potential form the standard table.

$E^0_{[Ag^{+}/Ag]}=+0.80V$

$E^0_{[Cu^{2+}/Cu]}=+0.34V$

In this cell, the component that has lower standard reduction potential gets oxidized and that is added to the anode electrode. The second forms the cathode electrode.

The balanced two-half reactions will be,

Oxidation half reaction (Anode) : $Cu(s)\rightarrow Cu^{2+}(aq)+2e^-$

Reduction half reaction (Cathode) : $Ag^{+}(aq)+e^-\rightarrow Ag(s)$

Thus the overall reaction will be,

$Cu(s)+2Ag^{+}(aq)\rightarrow Cu^{2+}(aq)+2Ag(s)$

From this we conclude that, 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

Hence, the 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

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3 years ago

1. What is a food web?

Anuta_ua [19.1K]

Answer:

a producer and consumer relationship how several food chains and related.

5 0

2 years ago

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The specific heat of copper metal is 0. 385 J/(g °C). How much energy must be added to a 35. 0-gram sample of copper to change t

Rus_ich [418]

The amount of heat required for changing the temperature of copper has been 606 J. Thus, option B is correct.

Specific heat has been defined as the amount of heat required to raise the temperature of 1 gram of substance by 1 degree Celsius.

The heat required to raise the temperature has been expressed as:

$\rm Heat=mass\;\times\;specific\;heat\;\times\;Change\;in\;temperature$