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CaHeK987 [17]
2 years ago
14

What elements are in SC14

Chemistry
1 answer:
zheka24 [161]2 years ago
5 0
Element Symbol Atomic weight # Mass percent
Sulfur S 32.065 1 16.0153
Carbon C 12.0107 14 83.9847
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And I living organism what is a tissue
Leviafan [203]
It is an ensemble of similar cells
4 0
2 years ago
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An Argon laser gives off pulses of green light (wavelength = 514 nm). If a single pulse from the laser has a total energy of 10.
svetoff [14.1K]

Answer:

n=2.59\times 10^{16} photons

Explanation:

E=n\times \frac{h\times c}{\lambda}

Where,  

n is the number of photons

h is Plank's constant having value 6.626\times 10^{-34}\ Js

c is the speed of light having value 3\times 10^8\ m/s

\lambda is the wavelength of the light

Given that, wavelength = 514 nm = 514\times 10^{-9}\ m

Energy = 10.0 mJ = 0.01 J ( 1 mJ = 0.001 J )

Applying the values as:-

0.01=n\times \frac{6.626\times 10^{-34}\times 3\times 10^8}{514\times 10^{-9}}

\frac{19.878n}{10^{17}\times \:514}=0.01

n=2.59\times 10^{16} photons

7 0
2 years ago
What is the molarity of a 10 L solution containing 5.0 moles of solute?
Setler79 [48]
Molarity = Moles of solute/ L(liters) of solution

So let's plug in the information. 

5.0 moles/10L = 0.5 M


3 0
2 years ago
Read 2 more answers
Calculate the number of grams of nitrogen dioxide that are produced from 4 moles of nitric oxide
miv72 [106K]

Answer:

hope this help by the way found off of yahoo

Explanation:

Calculate the number of grams of nitrogen dioxide that are produced from

4 moles of nitric oxide.

2NO(g) + O2(g) -->2NO2(g)

I really need help with this... I need to know how to work it too... I can balance it out but not sure about grams...  This is it balanced out with 4 moles of nitric oxide

4NO(g) + 2O2(g) ->4NO2(g) please help and explain i want to learn this

6 0
3 years ago
Given 3.4 grams of x compound with a molar mass of 85 g and 4.2 grams of y compound with a molar mass of 48 g How much of compou
Ulleksa [173]

Answer:

4.36~g~XY

Explanation:

In this case, we can start with the reaction:

2X + Y_2~->~2XY

If we check the reaction, we will have 2 X and Y atoms on both sides. So, <u>the reaction is balanced</u>. Now, the problem give to us two amounts of reagents. Therefore, we have to find the <u>limiting reagent</u>. The first step then is to find the moles of each compound using the <u>molar mass</u>:

3.4~g~X\frac{1~mol~X}{85~g~X}=0.04~mol~X

4.2~g~Y_2\frac{1~mol~Y_2}{48~g~Y_2}=0.0875~mol~Y_2

Now, we can <u>divide by the coefficient</u> of each compound (given by the balanced reaction):

\frac{0.04~mol~X}{1}=~0.04

\frac{0.0875~mol~Y_2}{2}=0.04375

The smallest value is for "X", therefore this is our <u>limiting reagent</u>. Now, if we use the <u>molar ratio</u> between "X" and "XY" we can calculate the moles of XY, so:

0.04~mol~X\frac{2~mol~XY}{2~mol~X}=0.04~mol~XY

Finally, with the molar mass of "XY" we can calculate the grams. Now, we know that 1 mol X = 85 g X and 1 mol Y_2 = 48 g Y_2 (therefore 1 mol Y = 24 g Y). With this in mind the <u>molar mass of XY</u> would be 85+24 = 109 g/mol. With this in mind:

0.04~mol~XY\frac{109~g~XY}{1~mol~XY}=4.36~g~XY

I hope it helps!

6 0
3 years ago
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