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maks197457 [2]
3 years ago
5

How many molecules is 0.360 mole of water?

Chemistry
1 answer:
Nikitich [7]3 years ago
4 0

Answer: 2.17 x 10^23 molecules

Explanation:

1mole of H2O contains 6.02x10^23 molecules.

Therefore 0.360mole of H2O will contain = 0.36 x 6.02x10^23 = 2.17 x 10^23 molecules

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g A and B are both non-volatile molecular compounds. Substance A has a greater molar mass than substance B. If 50 g of substance
Doss [256]

Answer:

The correct answer is - option D.  the boiling point of solution A will be lower than the boiling point of solution B

Explanation:

Colligative properties such as a decrease in the freezing point of the solution, increase in the boiling point of substance, decrease in Lowering of vapor pressure, and other properties depend upon the number of molecules only.

In the given solution the equal amount of two solutions are mixed that is 50 grams however due to the difference in the molecular mass so the atoms present in both solution A and B will be different. It is known that the number of atoms of a substance is inversely proportional to the molecular mass of the particular substance.

As it is given that Solution B has a low molecular mass which means it has a high number of atoms that means its boiling point will be higher than solution A.

8 0
2 years ago
For a particular redox reaction, NO-2 is oxidized to NO-3 and Ag+ is reduced to Ag . Complete and balance the equation for this
Salsk061 [2.6K]

The following are the steps  to complete and balnce the equation for the given reaction

<u>Explanation:</u>

We are given, NO2– is oxidized to NO3– and Ag is reduced to Ag

NO2– + Ag+ -----> NO3– + Ag(s)

Step 1) Assign the oxidation state to each element reaction

NO2– + Ag+ -----> NO3– + Ag(s)

N= +3                           N = +5                        

O = -2                            O = -2

Ag = +1                         Ag = 0

NO2– -----> NO3– ………oxidation half reaction

Ag+ -----> Ag(s) ……….reduction half reaction

Step 2) Balance the element other than O and H

     NO2– -----> NO3–

     Ag+ -----> Ag(s)

Step 3) Balance the O by adding 1 H2O for 1 O

     NO2– + H2O -----> NO3–

     Ag+ -----> Ag(s)

Step 4) Balance the H by adding H+

    NO2– + H2O -----> NO3– + 2H+

     Ag+ -----> Ag(s)

Step 5) Balance the charge by adding electron

    NO2– + H2O -----> NO3– + 2H+ + 2e-

     Ag+ + 1e------> Ag(s)

Step 6) Balance the electron in both half reaction

    NO2– + H2O -----> NO3– + 2H+ + 2e-

     2 Ag+ + 2e------> 2 Ag(s)

3 0
3 years ago
What occurs when Cr^3+ ions are reduced to Cr^2+ ions?
DiKsa [7]
D:

When electrons are gained, the charge of the atom decreases.

When you are given an atom with a charge, the oxidation of that atom is the charge. So by going from a Cr^3+ (Oxidation Number = 3) to a Cr^2+ (Oxidation Number = 2), the Oxidation Number thus decreases.
7 0
3 years ago
Show how acid and base given below dissociates in water​
Akimi4 [234]

Answer:

HOME is acid

KOH is base

5 0
3 years ago
An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0025 M O2. At this temperature, Kc
pantera1 [17]

Answer:

5.35 *10^{-4}M

Explanation:

Equation for the reaction is as follows:

2CO_{(g)}      +      O_{2(g)}        ⇄       2CO_{2(g)}

By Applying the ICE Table; we have

                             2CO_{(g)}      +      O_{2(g)}        ⇄       2CO_{2(g)}

Initial                      x                  0.0025 M              0.0010 M

Change                  0                       0                            0

Equilibrium             x                  0.0025 M              0.0010 M

K_c =\frac{[CO_2]^2}{[CO]^2[O_2]}

Given that K_c = 1.4*10^2 ; Then:

1.4 *10^2 = \frac{(0.001)^2}{(x)^2(0.025)}

1.4 *10^2*0.025 = \frac{(0.001)^2}{(x)^2}

3.5 =( \frac{(0.001)}{(x)})^2

\sqrt {3.5} = \sqrt {( \frac{(0.001)}{(x)} )^2}

1.87=\frac{(0.001)}{(x)}

(x)= \frac{(0.001)}{1.87 }

x = 5.35 *10^{-4}M

∴ The equilibrium concentration of CO = x = 5.35 *10^{-4}M

7 0
3 years ago
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