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Dafna11 [192]
3 years ago
10

What molarity is prepared when a solution contains 0.277 moles of calcium bromide in 500 mL of solution (must change mL to Liter

s)? *
Chemistry
1 answer:
Vladimir79 [104]3 years ago
5 0

Answer:

0.554M of Calcium Bromide

Explanation:

Molarity by defintion is #of moles of something/litres of solution.

Therefore, here, we have 0.277 moles of calcium bromide and 500mL (divide 500ml by 1000 to go from mL to L because for every 1L there's 1000mL) or 0.5L.

Molarity= 0.277/0.5 = 0.554M of Calcium Bromide

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Elanso [62]

Explanation:

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There are many misconceptions surrounding the Big Bang theory. For example, we tend to imagine a giant explosion. Experts however say that there was no explosion; there was (and continues to be) an expansion. Rather than imagining a balloon popping and releasing its contents, imagine a balloon expanding: an infinitesimally small balloon expanding to the size of our current universe. Another misconception is that we tend to image the singularity as a little fireball appearing somewhere in space. According to the many experts however, space didn't exist prior to the Big Bang. Back in the late '60s and early '70s, when men first walked upon the moon, "three British astrophysicists, Steven Hawking, George Ellis, and Roger Penrose turned their attention to the Theory of Relativity and its implications regarding our notions of time. In 1968 and 1970, they published papers in which they extended Einstein's Theory of General Relativity to include measurements of time and space. According to their calculations, time and space had a finite beginning that corresponded to the origin of matter and energy. I also know that there was a Big Bang is the fact that as things are moving closer to you the waves get compressed and as they are moving away from you the waves get stretched out. With light the shorter waves are the blue and the longer ones are the red and the further away a galaxy is the more red shifted it is indicating that the galaxies are all moving away from each other indicating that the universe was once much smaller and that at one time it was a singularity, which expanded until it got to the size it is today.

3 0
3 years ago
A major source of today's medicines
Arada [10]
A major source is coal
5 0
3 years ago
On a mission to a newly discovered planet, an astronaut finds chlorine abundances of 13.85 % for 35Cl and 86.15 % for 37Cl. What
topjm [15]

Answer : The atomic mass of chlorine is, 36.723 amu

Explanation :

Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.

Formula used to calculate average atomic mass follows:

\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i

As we are given that,

Mass of 35-Cl isotope = 35 amu

Percentage abundance of 35-Cl isotope = 13.85 %

Fractional abundance of 35-Cl isotope = 0.1385

Mass of 37-Cl isotope = 37 amu

Percentage abundance of 37-Cl isotope = 86.15 %

Fractional abundance of 37-Cl isotope = 0.8615

Now put all the given values in above formula, we get:

\text{Average atomic mass }=[(35\times 0.1385)+(37\times 0.8615)]

\text{Average atomic mass }=36.723amu

Therefore, the atomic mass of chlorine is, 36.723 amu

6 0
4 years ago
How many moles of Boron are present in 20g of borax (sodium tetraborate)?​
stira [4]
20 grams of borax contains (20.0g) / (201 g mol -1) =0.10 mol of borax.

Therefore 0.40 mol of borax
5 0
3 years ago
A 1.40 L sample of O2 at 645 Torr and 25 °C, and a 0.751 L sample of N2 at 1.13 atm and 25 °C, are both transferred to the same
anyanavicka [17]

Answer:

  • P(O₂) = 0.595 atm
  • P(N₂) = 0.424 atm
  • Total Pressure = 1.019 atm

Explanation:

To solve this problem we use PV=nRT for both gases in their containers, in order to <u>calculate the moles of each one</u>:

  • O₂:

645 Torr ⇒ 645 /760 = 0.85 atm

25°C ⇒ 25 + 273.16 = 298.16 K

0.85 atm * 1.40 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ *298.16 K

n = 0.0487 mol O₂

  • N₂:

1.13 atm * 0.751 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ *298.16 K

n = 0.0347 mol N₂

Now we can <u>calculate the partial pressure for each gas in the new container</u>, because the number of moles did not change:

  • O₂:

P(O₂) * 2.00 L = 0.0487 mol O₂ * 0.082 atm·L·mol⁻¹·K⁻¹ *298.16 K

P(O₂) = 0.595 atm

  • N₂:

P(N₂) * 2.00 L = 0.0347 mol N₂ * 0.082 atm·L·mol⁻¹·K⁻¹ *298.16 K

P(N₂) = 0.424 atm

Finally we add the partial pressures of all gases to <u>calculate the total pressure</u>:

  • Pt = 0.595 atm+ 0.424 atm = 1.019 atm
6 0
4 years ago
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