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DochEvi [55]
3 years ago
14

A vector always consists of

Chemistry
1 answer:
bija089 [108]3 years ago
7 0
Hope this helps <span>A vector always consists of a direction and magnitude. F</span>
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Do elements have DNA?
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Not most elements have DNA, only five "elements" have DNA. <span>The five "elements" are Carbon, Oxygen, Hydrogen, Nitrogen and Phosphorus. Good luck with your question I hope this is what you were looking for.</span>
6 0
3 years ago
You place a balloon in a closed chamber at STP. When the balloon doubles in size, what happens to the chamber pressure? A.) The
larisa86 [58]
If you increase the volume the pressure will decrease.  so the best answer is C
4 0
3 years ago
Read 2 more answers
In an ionic bond:
Fynjy0 [20]

In an ionic bond :

=》B. one atom accepts electrons from another.

in this bond an atom ( <em><u>metallic</u></em> ) loses its electrons and another atom ( <em><u>non- metallic</u></em> ) accepts the electrons, and since there isn't the equal positive and negative charges in the atoms, they forms <em><u>cations</u></em> ( +ve charge ) and <em><u>anions </u></em>( -ve charge )

and get stacked or <em><u>attracted</u></em> to each other by strong <em><u>electrostatic force</u></em>.

4 0
3 years ago
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A chemist prepares a solution of sodium thiosulfate by measuring out of sodium thiosulfate into a volumetric flask and filling t
marshall27 [118]

Mass of sodium thiosulfate Na_{2}S_{2}O_{3} is 110. g

Volume of the solution is 350. mL

Calculating the moles of sodium thiosulfate:

110. g Na_{2}S_{2}O_{3} * \frac{1 mol Na_{2}S_{2}O_{3}}{158.1 g Na_{2}S_{2}O_{3}} = 0.696 molNa_{2}S_{2}O_{3}

Converting the volume of solution to L:

350. mL * \frac{1 L}{1000 mL} = 0.350 L

Finding out the concentration of solution in molarity:

\frac{0.696 mol}{0.350 L} =  1.99 mol/L

4 0
3 years ago
0.10 M potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2. What is the Ag+ concentrati
erastova [34]

Answer:

[Ag^{+}]=4.2\times 10^{-2}M

Explanation:

Given:

[AgNO3] = 0.20 M

Ba(NO3)2 = 0.20 M

[K2CrO4] = 0.10 M

Ksp of Ag2CrO4 = 1.1 x 10^-12

Ksp of BaCrO4 = 1.1 x 10^-10

BaCrO_4 (s)\leftrightharpoons  Ba^{2+}(aq)\;+\;CrO_{4}^{2-}(aq)

Ksp=[Ba^{2+}][CrO_{4}^{2-}]

1.2\times 10^{-10}=(0.20)[CrO_{4}^{2-}]

[CrO_{4}^{2-}]=\frac{1.2\times 10^{-10}}{(0.20)}= 6.0\times 10^{-10}

Now,

Ag_{2}CrO_4(s) \leftrightharpoons  2Ag^{+}(aq)\;+\;CrO_{4}^{2-}(aq)

Ksp=[Ag^{+}]^{2}[CrO_{4}^{2-}]

1.1\times 10^{-12}=[Ag^{+}]^{2}](6.0\times 10^{-10})

[Ag^{+}]^{2}]=\frac{1.1\times 10^{-12}}{(6.0\times 10^{-10})}= 1.8\times 10^{-3}

[Ag^{+}]=\sqrt{1.8\times 10^{-3}}=4.2\times 10^{-2}M

So, BaCrO4 will start precipitating when [Ag+] is 4.2 x 1.2^-2 M

                       

7 0
3 years ago
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