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Thepotemich [5.8K]
3 years ago
14

Help! help! plz............

Chemistry
1 answer:
zhuklara [117]3 years ago
8 0
There the picture is the answer from the internet

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A chemist determined by measurements that 0.050 moles of tin participated in a chemical reaction. Calculate the mass of tin that
stepladder [879]

Answer:

Explanation:

MM of I2 = 2 (127 g) = 254 g/mol

0.065 mol I2 x 254g I₂/ 1 mol I₂  = 16.5 g I2

8 0
2 years ago
Read 2 more answers
What could be the fourth quantum number of a 1s^2 electron be?
Bumek [7]

The forth quantum number is Spin quantum number and the value of Spin Quantum Number of 1s² will be +1/2. Therefore, the correct option is (B) option

<h3>What is Spin Quantum Number ?</h3>

It describes the orientation of the electron spin (rotation) in space.

In the given case of 1s² configuration,

since, the Quantum numbers are known as:

  • Principal quantum number (n) which cannot be zero.

       The allowed values of n are therefore 1, 2, 3, 4, and so on.

  • Angular quantum number (l) is able to be any integer between 0  

       and n-1.

       Therefore, for example, If n = 1, l will be 0,

                                                If n = 2, l can be either 0 or 1.

  • Magnetic quantum number (m) is able to be any integer between -l and +l.    

       Therefore, for example, If l = 3, m can be either -3 to +3.

  • Spin Quantum Number (ms): Ms = +½ or -½  accounts for the orientation of the spin axis of an electron as it is able to spin in only one of two directions.

Thus, since the fourth quantum number is Ms, spin, we infer that the answer is (B) option ie, Ms = +1/2 because it represents the positive spin on 1s².

Learn more about Quantum Number Here ;

brainly.com/question/15325270

#SPJ1

6 0
2 years ago
What makes your pulse? Explain​
Serga [27]
Blood flowing into and out your heart makes your pulse
6 0
2 years ago
I need help with this anyone?
valkas [14]
Just look it up on goog^le or a chart
5 0
3 years ago
Can someone help me? <br><br>-just check my latest question.. thanks... ​
Harman [31]

Explanation:

{\boxed{ \fbox{ \fbox{ \fbox{ \red{hello}}}}}}

{\boxed{ \fbox{ \fbox{ \fbox{ \green{hello}}}}}}

{\boxed{ \fbox{ \fbox{ \fbox{ \pink{hello}}}}}}

▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬\mathscr \fcolorbox{blue}{green}{BE \: BRAINLY}▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬\mathscr \fcolorbox{blue}{blue}{BE \: BRAINLY}▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬\mathscr \fcolorbox{blue}{red}{BE \: BRAINLY}▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬\mathscr \fcolorbox{blue}{gray}{BE \: BRAINLY}▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬

\mathscr \fcolorbox{blue}{pink}{BE \: BRAINLY}

<h2>yes can you. do this</h2>
7 0
2 years ago
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