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Lena [83]
3 years ago
5

Which doesn't belong in the group?

Chemistry
1 answer:
ivann1987 [24]3 years ago
6 0
Magnetite because it is an iron ore while the rest are magnets or have to do with magnetism.
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1. Which of these has only one component?
Phantasy [73]
1. Element
2. Sugar and window cleaner
3. Heterogeneous mixture.
8 0
3 years ago
Rank the following in order from most acidic to least acidic. sample pH bleach 12.5 coffee 4.2 rainwater 5.4 soap 10.1 (1 point)
Ainat [17]
Hope this helps you.

6 0
3 years ago
The pressure at the center of the earth is probably greater than 3x106 atm, and the temperature there is about 4000 °C. What is
andrezito [222]

Answer:

The change in the Gibbs function of reaction on going from crust to core, dG=291442.4 J/mol

Explanation:

dG=vdp-sdT

Where T is the temperature .

P is the pressure.

S is entropy

V= 1cm3 =10-6 m3

P= 3*10∧6 atm = 3*10∧11 pa

The temperature at the center of the earth, Tc = 4*103 °C. : The temperature at the sufrace (crust) of the earth, Ts =298K.

Subistuting the values

dG = (10-6 *(3*1011-105) - (2.1(4373-298))

dG=291442.4 J/mol.

7 0
3 years ago
A sample of oxygen gas was collected via water displacement. since the oxygen was collected via water displacement, the sample i
mylen [45]

The sample of oxygen gas was collected through water displacement. So, the gas collected will be a mixture of oxygen and water vapor.

Given that the total pressure of the mixture of gases containing oxygen and water vapor = 749 Torr

Vapor pressure of pure water at 26.4^{0}C=25.81mmHg

                               = 25.81 mmHg*\frac{1 Torr}{1 mmHg} =25.81 Torr

According to Dalton's law of partial pressures,

Total pressure = Partial pressure of Oxygen gas + Partial pressure of water

  749 Torr = Partial pressure of Oxygen gas + 25.81 Torr

Partial pressure of Oxygen gas = 749 Torr - 25.81 Torr =  723.19 Torr

Therefore the partial pressure of Oxygen gas in the mixture collected will be 723.19 Torr


6 0
3 years ago
How much mercury and oxygen could be obtained from 21.7g of mercury (II) oxide
Musya8 [376]

20.06 g of Hg  and 1.6 g of O₂

<u>Explanation:</u>

To Find:

Number of Mercury and oxygen that can be obtained from 21.7 g of HgO

First we have to write the balanced equation for the decomposition reaction of Mercury(II) oxide as,

2 HgO (s) → 2Hg(l) + O₂ (g)

21.7 g of HgO  = \frac{21.7 g}{216.59  g / mol}  

                         = 0.1 mol of HgO.

As per the above equation, we can find the mole ratio between HgO and Hg is 1: 1 and that of HgO and oxygen is 2:1 .

So amount of Hg produced = 0.1 mol × 200.59 g / mol ( molar mass of Hg)

                                                 = 20.06 g of Hg

Amount of oxygen produced = 0.05  mol × 32 g/ mol = 1.6 g of O₂

Thus it is clear that 20.06 g of Hg  and 1.6 g of O₂  is obtained from 21.7 g of HgO

7 0
3 years ago
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