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Roman55 [17]
2 years ago
8

Which solution whose POH is 12

Chemistry
1 answer:
lesya692 [45]2 years ago
3 0

Answer:

d

Explanation:

H3O =1×10_12=12 ooh is 12

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What happens to the particles during condensation
Paraphin [41]

Answer:

molecus in a gas cool down

Explanation:

the molecules lose heat and energy do they slow down they move closer to other molecules and form a liquid

8 0
3 years ago
HELP!!!! ASAP!!! Fast please !!! Is this A. Closed parallel circuit B. Closed series circuit C. Open series circuit D. Open para
tatuchka [14]
Closed parallel circuit.<span />
7 0
3 years ago
A 1.00 L flask is filled with 1.15 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pres
tatiyna

Answer:

The partial pressure of argon in the flask = 71.326 K pa

Explanation:

Volume off the flask = 0.001 m^{3}

Mass of the gas = 1.15 gm = 0.00115 kg

Temperature = 25 ° c = 298 K

Gas constant for Argon R = 208.13 \frac{J}{kg k}

From ideal gas equation P V = m RT

⇒ P = \frac{m R T}{V}

Put all the values in above formula we get

⇒ P = \frac{0.00115}{0.001} × 208.13 × 298

⇒ P = 71.326 K pa

Therefore, the partial pressure of argon in the flask = 71.326 K pa

4 0
3 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
Using the balanced equation N2+O2=2NO, how many grams of NO can be produced when 25.0 grams of N react?
Oxana [17]

Answer:

53.55gNO

Explanation:

Hello there!

In this case, according to the given chemical reaction, it is possible for us to calculate the produced grams of nitrogen monoxide by starting with 25.0 g of nitrogen via their 1:2 mole ratio and the molar masses of 30.1 g/mol and 28.02 g/mol, respectively and by some stoichiometry:

=25.0gN_2*\frac{1molN_2}{28.02gN_2}*\frac{2molNO}{1molN_2}*\frac{30.01 gNO}{1molNO}\\\\=53.55gNO

Best regards!

8 0
3 years ago
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