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m_a_m_a [10]
3 years ago
6

EASY

Chemistry
2 answers:
kogti [31]3 years ago
7 0

Answer:

THE SAME NUMBER OF PROTONS

Explanation:

Anestetic [448]3 years ago
3 0
The same number of protons
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Why copper should not be disposed of in landfill sites?
Dafna1 [17]
Copper is a heavy metal that can harm many people. This process of heavy metals building in your body is called bioaccumulation and the process of this building in the food chain is called biomagnification. Its hard to rid of this heavy metal because it is very dense, therefore, cannot breakdown in our bodies. Heavy metals get consumed by producers and then reach to the top of the pyramid (us) so we have the highest risk of getting diseases and so on. Make sure you explain that heavy metals get passed from industrial purposes where companies do not dispose of waste properly.
Source: Exam as well
Good luck!  
4 0
3 years ago
Read 2 more answers
18.2L of gas at 95°C and 760 torr is placed in a 15L container at 80 degrees * C ; what is the new pressure ?
romanna [79]

Answer:

884.56 torr

Explanation:

Formula: \frac{P_{1}V_{1} }{T_{1}} = \frac{P_{2}V_{2} }{T_{2}}

P = Pressure

V = Volume

T = Temperature in kelvin (Celsius + 273.15)

\frac{(760)(18.2) }{368.15} = \frac{P(15) }{353.15}

P = \frac{(760)(18.2)(353.15) }{(368.15)(15)}

P = 884.56169

4 0
3 years ago
Is petroleum potential or kinetic energy
Sav [38]
Petroleum is a potential.
yeah that's my guess.
8 0
3 years ago
An unknown element sample has 2 isotopes present. The first isotope has a mass of 6.017 amu and is
oksano4ka [1.4K]

Answer:

Calculating Atomic Mass

Change each percent abundance into decimal form by dividing by 100. Multiply this value by the atomic mass of that isotope. Add together for each isotope to get the average atomic mass.

Explanation:

have a nice day

8 0
2 years ago
For the reaction N2(g) + 2H2(g) → N2H4(l), if the percent yield for this reaction is 100.0%, what is the actual mass of hydrazin
barxatty [35]

Answer:

53.6 g of N₂H₄

Explanation:

The begining is in the reaction:

N₂(g) + 2H₂(g) → N₂H₄(l)

We determine the moles of each reactant:

59.20 g / 28.01 g/mol = 2.11 moles of nitrogen

6.750 g / 2.016 g/mol = 3.35 moles of H₂

1 mol of N₂ react to 2 moles of H₂

Our 2.11 moles of N₂ may react to (2.11 . 2) /1 = 4.22 moles of H₂, but we only have 3.35 moles. The hydrogen is the limiting reactant.

2 moles of H₂ produce at 100 % yield, 1 mol of hydrazine

Then, 3.35 moles, may produce (3.35 . 1)/2 = 1.67 moles of N₂H₄

Let's convert the moles to mass:

1.67 mol . 32.05 g/mol = 53.6 g

4 0
3 years ago
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