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Inessa [10]
4 years ago
12

Would someone please help?

Chemistry
1 answer:
sveta [45]4 years ago
3 0
The season that is starting is winter.
The answer to 21 is (4)
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A particle with charge +1 nC (a nanocoulomb is 1 10-9 C) is located at the origin. What is the electric field due to this partic
Zolol [24]

Answer:

E=35.97\frac{V}{m}

Explanation:

The electric field of a point charge can be calculated using the next equation:

E=\frac{1}{4\pi \epsilon_0} \frac{Q}{r^2}

Where:

\epsilon_0=Absolute\hspace{3}permittivity\hspace{3}of\hspace{3}free\hspace{3}space\approx 8.85\times 10^{-12} \\Q=Charge\hspace{3}magnitude\\r=Distance

The distance can be calculated as:

r=\sqrt{0.5^2+0^2+0^2} =0.5

Using the data provided by the problem:

E=\frac{1}{4\pi (8.85\times 10^{-12}) } \frac{1\times 10^{-9} }{0.5^2} =35.96721878\approx35.97V/m

8 0
4 years ago
If you burn yourself in lab you should?
VladimirAG [237]

Answer:

B. Tell the instructor

Explanation:

Always to the instructor about any accidents happens in a lab.

5 0
3 years ago
this is my third time asking this,,, HELPPPPPP PLZZZz i'll mark brainliest! Infrared (IR) and ultraviolet (UV) light. But above
mezya [45]

Answer:it would not cause any effect because its blocking it. Basically u could say that what would happen is that no effect was happening cuz of the blocking.

Explanation:

5 0
3 years ago
How many grams of Cl2 are consumed to produce 12.0 g of KCl?
Alla [95]

The reaction is:

Cl2 + 2 KBr --> 2 KCl + Br2

Moles of KCl is

n = m /M = 12 /74 = 0.16 mol

As, twice the moles of KCl is producing from 1 mol of chlorine

mole of Cl2 = 0.16 /2 = 0.08 mol

Mass of Cl2

m /70 = 0.08 = 5.6 g

Hence, 5.6 g mol Cl2 consumed to produce KCl

7 0
3 years ago
5. Calculate the mass percent of carbon in C3H8
Anuta_ua [19.1K]

Answer: How to calculate the mass percent by using these instructions

1.The molar mass is the mass of a given chemical element or chemical compound (g) divided by the amount of substance (mol).

2.The molar mass of a compound can be calculated by adding the standard atomic masses (in g/mol) of the constituent atoms.

Explanation:

7 0
3 years ago
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