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yanalaym [24]
3 years ago
5

Which of the following are examples of strong electrolytes?

Chemistry
1 answer:
mihalych1998 [28]3 years ago
5 0
B. Strong acids and Strong bases 
Electrolytes are acids bases and salts
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It says draw a ring around all the objects that will be attracted to a magnet the one there are : a 2p coin,cobalt,an aluminium
Katen [24]

Answer: do

Explanation:

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When did the mass extinctions happen
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Out of the five major mass extinction, one is Cretaceous-Tertiary extinction (K-T extinction). It happened 66 million years ago marked by the end of the Cretinous period.
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A student knows that hydrogen (H) atoms and oxygen (O) atoms combine to form water (H2O). The student correctly predicts that hy
marusya05 [52]

Answer:

A

Explanation:

They both need to lose 2 electrons to form ions

6 0
3 years ago
Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H2O2
zalisa [80]

Answer:

23.0733 L

Explanation:

The mass of hydrogen peroxide present in 125 g of 50% of hydrogen peroxide solution:

Mass=\frac {50}{100}\times 125\ g

Mass = 62.5 g

Molar mass of H_2O_2 = 34 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus, moles are:

moles= \frac{62.5\ g}{34\ g/mol}

moles= 1.8382\ mol

Consider the given reaction as:

2H_2O_2_{(aq)}\rightarrow2H_2O_{(l)}+O_2_{(g)}

2 moles of hydrogen peroxide decomposes to give 1 mole of oxygen gas.

Also,

1 mole of hydrogen peroxide decomposes to give 1/2 mole of oxygen gas.

So,

1.8382 moles of hydrogen peroxide decomposes to give \frac {1}{2}\times 1.8382 mole of oxygen gas. Moles of oxygen gas produced = 0.9191 molGiven: Pressure = 746 torr
The conversion of P(torr) to P(atm) is shown below:
[tex]P(torr)=\frac {1}{760}\times P(atm)

So,

Pressure = 746 / 760 atm = 0.9816 atm

Temperature = 27 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = (27 + 273.15) K = 300.15 K

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.9816 atm × V = 0.9191 mol × 0.0821 L.atm/K.mol × 300.15 K

<u>⇒V = 23.0733 L</u>

8 0
3 years ago
Determine the mass of 5.20 moles of c6h12
Gwar [14]
Mass is equal to moles x molar mass, and the molar mass of C6H12 is 84, therefore the mass is 436.8 g, but 437 rounded to correct significant figures
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