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exis [7]
2 years ago
13

What the common uses for Bohrium?

Chemistry
2 answers:
weqwewe [10]2 years ago
6 0

Answer:

look it up?

Explanation:

lora16 [44]2 years ago
5 0

Answer:

Explanation:

Bohrium's most stable isotope, bohrium-270, has a half-life of about 1 minute. It decays into dubnium-266 through alpha decay. Since only a few atoms of bohrium have ever been made, there are currently no uses for bohrium outside of basic scientific research.

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Find the kinetic energy of the horse using KE=1/2 mv².
Dmitry [639]
KE=6,250Joules
You plug in your given numbers and remember to square 5 because that’s the speed
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3 years ago
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Cho recorded the weather in her town for a week. She wrote down her observations in the table below. Mon Tue Wed Thu Fri Sat Sun
SIZIF [17.4K]

Answer:

If this trend continues, the following week will be cooler, and a large amount of rain will fall.

Explanation:

Patterns and trends can often be found in data sets. During the week that Cho recorded the weather, the temperatures consistently dropped by one to four degrees each day. At the end of the week, the amount of precipitation increased daily.

6 0
3 years ago
Which 'tropic' is located in the southern hemisphere?
butalik [34]
Its Southern Hemisphere counterpart, marking the most southerly position at which the Sun can be directly overhead, is the Tropic of Capricorn. These tropics are two of the five major circles of latitude that mark maps of the Earth, besides the Arctic and Antarctic Circles and the Equator.
6 0
3 years ago
How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 4.46 atm and 45°C in the reaction shown below?
natka813 [3]

Answer:

8.1433 g of XeF₆  are required.

Explanation:

Balanced chemical equation;

XeF₆ (s) + 3H₂ (g)   →  Xe (g) + 6HF (g)

Given data:

Volume of hydrogen = 0.579 L

Pressure = 4.46 atm

Temperature = 45 °C (45+273= 318 k)

Solution:

First of all we will calculate the moles of hydrogen

PV = nRT

n = PV/ RT

n = 4.46 atm × 0.579 L / 0.0821 atm. dm³. mol⁻¹. K⁻¹ × 318 K

n = 2.6 atm . L / 26.12 atm. dm³. mol⁻¹

n = 0.0995 mol

Mass of hydrogen:

Mass = moles × molar mass

Mass =  0.0995 mol × 2.016 g/mol

Mass =  0.2006 g

Now we will compare the moles of hydrogen with XeF₆ from balance chemical equation.

                                         H₂   :  XeF₆

                                          3    :    1

                                 0.0995   : 1/3× 0.0995 = 0.0332 mol

Now we will calculate the mass of XeF₆.

Mass = moles × molar mass

Mass = 0.0332 mol × 245.28 g/mol

Mass = 8.1433 g

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