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3 years ago

Which is heavier einsteinium (Es) or europium (Eu)

Chemistry

1 answer:

Maksim231197 [3]3 years ago

3 0

Answer:

Einsteinium is heavier

Explanation:

Atomic weight is what we are referring to when figuring out how heavy an element is and is measured in amu (atomic mass units)

(This is also the same as the molar mass how heavy 6.022 x 10^23 atoms of a substance or element is which is measured in grams)

The atomic weight of an element can be found on a periodic table.

Europium has an atomic mass of approximately 152 amu (atomic mass units)

Einsteinium has an atomic mass of approximately 252 amu.

Einsteinium has a higher atomic weight so it's heavier.

There's another easier way of going about it where you don't even have to think about the actual number and basically just look at the element's atomic number and position on the periodic table.

Eu is 63

Es is 99

As the atomic number increases on the periodic table this means it's number of protons is greater.

Protons lie in the nucleus which has most of the atom's weight so the more protons the heavier it is.

Einsteinium has a higher atomic number meaning it has more protons so we can assume it's the heavier one.

Hope this helps!

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If the concentrated form of blood expander is 9.0 mol/L and one of your companions, a nurse, tells you that you need to have a f

I am Lyosha [343]

Answer:

0.032 L or 32 mL

Explanation:

Use the dilution equation M1V1 = M2V2

M1 = 9.0 M

V1 = This is what we're looking for.

M2 = 0.145 M

V2 = 2 L

Solve for V1 --> V1 = M2V2/M1

V1 = (0.145 M)(2 L) / (9.0 M) = 0.032 L

3 0

3 years ago

23.5 L of h2 is stored at a pressure of 58.7 Kpa what volume would the gas take up at stp

stepan [7]

Answer:- 13.6 L

Solution:- Volume of hydrogen gas at 58.7 Kpa is given as 23.5 L. It asks to calculate the volume of hydrogen gas at STP that is standard temperature and pressure. Since the problem does not talk about the original temperature so we would assume the constant temperature. So, it is Boyle's law.

Standard pressure is 1 atm that is 101.325 Kpa.

Boyle's law equation is:

$P_1V_1=P_2V_2$

From given information:-

$P_1$ = 58.7 Kpa

$V_1$ = 23.5 L

$P_2$ = 101.325 Kpa

$V_2$ = ?

Let's plug in the values and solve it for final volume.

$58.7Kpa*23.5L=101.325Kpa*V_2$

On rearranging the equation for $V_2$

$V_2=\frac{58.7Kpa*23.5L}{101.325Kpa}$

$V_2$ = 13.6 L

So, the volume of hydrogen gas at STP for the given information is 13.6 L.

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2 years ago

1.What does the Law of Conservation of Energy tells us?

lorasvet [3.4K]

1. Energy can neither be created or destroyed.
2. Conduction. Putting a pot of water on a hot burner. Convection. Putting your wet shoes over an air vent to dry them quicker. Radiation. Sitting in front of the fire to warm your hands up.
3. renewable sources can be used again and again, but non renewable sources cannot.
4. I would recommend solar energy. I think solar energy should be considered because solar energy can be reused, and also because they can use it to power their houses and they wouldn't need fossil fuels to do so.
5. Turn off the lights and open the windows during the day and if something is left plugged into the wall and it is not being used, unplug it.

hope I could help!

4 0

3 years ago

What mass would release 2620J of heat when cooled 50 degrees C?

OverLord2011 [107]

the answer is B)12.5

7 0

3 years ago

Read 2 more answers

How many moles are in 7.00E24 atoms of Ca?

iris [78.8K]

Explanation:

In chemistry, a mole is the base unit of the amount of substance in a system containing elementary entities (atoms, molecules, ions, electrons), and one mole of substance corresponds to the Avogadro's constant or $6.023 \ \times \ 10^{23}$ entities. The stoichiometry equation that relates the amount of substance into the measurement in moles is

$n \ = \ \displaystyle\frac{\alpha}{N_{A}}$ ,

where $n$ is the number of moles, $\alpha$ is the amount of substance and $N_{A}$ is the Avogadro's constant.

Therefore,

$n \ = \ \displaystyle\frac{7.00 \ \times \ 10^{24} \ \text{atoms}}{6.023 \ \times \ 10^{23} \ \text{atoms mol}^{-1}} \\ \\ n \ = \ 11.624 \ \text{mol}$ .

3 0

2 years ago