5.924 g
Step-by-step explanation:
The average weight of a boron atom is 10.811 atomic mass units (AMU). Therefore 3.3 x 10^23 atoms of boron will weight;
3.3 x 10^23 * 10.811 = 3.56763 x 10 ^ 24
One (1) gram = 6.022 x 1023 AMU. Therefore to convert AMU to grams;
3.56763 x 10 ^ 24 / 6.022 x 10^23
= 5.924 g
Learn More:
For more on atomic mass check out;
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Answer:
Step-by-step explanation:
In this item, we are asked to determine or calculate for the distance between the points A (1,4) and B(-3,-2)
The distance between the two points can be computed through the equation below.
d = sqrt ((x₂ - x₁)² + (y₂ - y₁)³)
We can choice whichever of the two points will have the first abscissa or the first ordinate. For the purpose of showing the solution here, it is assumed that A has the coordinates of (x₁,y₁) and B (x₂,y₂)
Substituting,
d = sqrt ((-3 - 1)² + (-2 -4)²)
d = 2√13
<em>ANSWER: 2√13 , ~7.21</em>
