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statuscvo [17]
3 years ago
10

Enter the net ionic equation for the reaction of AgNO3(aq)

Chemistry
1 answer:
mixas84 [53]3 years ago
6 0

Answer:

Explanation:

This is a typical double replacement or double decomposition reaction. In this kind of reaction, it involves the combination of ionic compounds which exchange their partners to form new compounds. Typical of these reaction is the formation of precipitates which are insoluble compounds.

The reaction equation is shown below:

 AgNO₃(_{aq} ) + K₂SO₄(_{aq} ) → 2KNO₃(_{aq} ) + AgSO₄(_{s} )

From the rule of solubility:

  • All trioxonitrate(v) salts are soluble
  • Salts of silver sulfates are slightly soluble. This will form the precipitate in the solution.

We can write the ionic equation as:

      Ag⁺(_{aq} ) + NO₃⁻(_{aq} ) + 2K⁺(_{aq} ) + SO₄²⁻(_{aq} ) → AgSO₄(_{s} ) + 2K⁺ + NO₃⁻(_{aq} )

The spectator ions or non-reactive ions are those ions that appears on both sides of the equation. These ions are the potassium and trioxonitrate ions. We cancel them out to give the net ionic equation of the reaction:

 Ag⁺(_{aq} ) + SO₄²⁻(_{aq} ) → AgSO₄(_{s} )

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<h3>Answer:</h3>

32.98°C

<h3>Explanation:</h3>

We are given the following;

Mass of Aluminium as 125 g

Initial temperature of Aluminium as 182°C

Mass of water as 265 g

Initial temperature of water as 22°C

We are required to calculate the final temperature of the two compounds;

First, we need to know the specific heat capacity of each;

Specific heat capacity of Aluminium is 0.9 J/g°C

Specific heat capacity of water is 4.184 J/g°C

<h3>Step 1: Calculate the Quantity of heat gained by water.</h3>

Assuming the final temperature is X°C

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Change in temperature, ΔT = (X-22)°C

therefore;

Q = 365 g × 4.184 J/g°C × (X-22)°C

    = (1527.16X-33,597.52) Joules

<h3>Step 2: Calculate the quantity of heat released by Aluminium </h3>

Using the final temperature, X°C

Change in temperature, ΔT = -(X°- 182°)C (negative because heat was lost)

Therefore;

Q = 125 g × 0.90 J/g°C × (182°-X°)C

  = (20,475- 112.5X) Joules

<h3>Step 3: Calculating the final temperature</h3>

We need to know that the heat released by aluminium is equal to heat absorbed by water.

Therefore;

(20,475- 112.5X) Joules = (1527.16X-33,597.52) Joules

Combining the like terms;

1639.66X = 54072.52

             X = 32.978°C

                = 32.98°C

Therefore, the final temperature of the two compounds will be 32.98°C

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It takes to break an iodine-iodine single bond. Calculate the maximum wavelength of light for which an iodine-iodine single bond
Zolol [24]

The given question is incomplete. The complete question is :

It takes 151 kJ/mol to break an iodine-iodine single bond. Calculate the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.

Answer:  793 nm

Explanation:

The relation between energy and wavelength of light is given by Planck's equation, which is:

E=\frac{hc}{\lambda}

where,

E = energy of the light  = 151 kJ= 151000 J   (1kJ=1000J)

N= moles = 1 = 6.023\times 10^{23}

h = Planck's constant  = 6.626\times 10^{-34}Js

c = speed of light  = 3\times 10^8m/s

\lambda = wavelength of light  = ?

Putting in the values:

151000J=\frac{6.023\times 10^{23}\times 6.626\times 10^{-34}Js\times 3\times 10^8m/s}{\lambda}

{\lambda}=7.93\times 10^{-7}m=793nm    1m=10^{-9}nm

Thus  the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon is 793 nm

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3 years ago
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