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ki77a [65]
3 years ago
5

Which product formed when MgO and H2O react together?

Chemistry
2 answers:
SIZIF [17.4K]3 years ago
5 0
<span>MgO + H</span>₂<span>O = Mg(OH)</span>₂


Mg(OH)₂ = <span>Magnesium hydroxide
</span>
hope this helps!

seropon [69]3 years ago
4 0
When MgO and H2O react they form Magnesium Hydroxide Mg(OH)2
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Do you think crystals formed in conditions that were stable or did they change often?
andreev551 [17]

Answer:

They were made in unstable conditions

Explanation: Im smarty pants

6 0
3 years ago
natural rubidium has the average mass of 85.4678 and is composed of isotopes 85 Rb(mass = 84.9117) and 87 Rb. The ratio of atoms
mote1985 [20]

Answer:

Mass of Rb-87 is 86.913 amu.

Explanation:

Given data:

Average mass of rubidium = 85.4678 amu

Mass of Rb-85 = 84.9117

Ratio of 85Rb/87Rb in natural rubidium = 2.591

Mass of Rb = ?

Solution:

The ration of both isotope is 2.591 to 1. Which means that for 2.591 atoms of Rb-85 there is one Rb-87.

For 100% naturally occurring Rb = 2.591 + 1 = 3.591

% abundance of Rb-85 = 2.591/ 3.591 = 0.722

% abundance of Rb-87 = 1 - 0.722= 0.278

84.9117 × 0.722 + X × 0.278 = 85.4678

61.306 + X × 0.278 = 85.4678

X × 0.278 = 85.4678 - 61.306

X × 0.278 = 24.1618

X =  24.1618 / 0.278

X = 86.913 amu

8 0
3 years ago
Which substance can be decomposed by a chemical change?<br> (1) Co (3) Cr(2) CO (4) Cu
kotykmax [81]
Answer: (2) CO

Co, Cr, and Cu are elements. Elements cannot be broken down by a chemical change, but compounds can. Since CO is a compound, it can be decomposed by a chemical change.
7 0
3 years ago
How many moles of helium gas are contained in a 4.0-L flask at STP?
mel-nik [20]
1.0 mole of gas at STP occupies 22.4 Litres.
4/0L / 22.4 L/mole = 0.179 moles He.
4 0
3 years ago
Read 2 more answers
If 20.0g of CO2 and 4.4g of CO2
Ksivusya [100]

The given question is incorrect. The correct question is as follows.

If 20.0 g of O_{2} and 4.4 g of CO_{2}  are placed in a 5.00 L container at 21^{o}C, what is  the pressure of this mixture of gases?

Explanation:

As we know that number of moles equal to the mass of substance divided by its molar mass.

Mathematically,   No. of moles = \frac{\text{mass}}{\text{molar mass}}

Hence, we will calculate the moles of oxygen as follows.

       No. of moles = \frac{\text{mass}}{\text{molar mass}}

     Moles of O_{2} = \frac{20.0 g}{32 g/mol}

                            = 0.625 moles

Now,   moles of CO_{2} = \frac{4.4 g}{44 g/mol}

                                      = 0.1 moles

Therefore, total number of moles present are as follows.

Total moles = moles of O_{2} + moles of CO_{2}

                    = 0.625 + 0.1

                    = 0.725 moles

And, total temperature  will be:

                    T = (21 + 273) K = 294 K

According to ideal gas equation,  

                         PV = nRT

Now, putting the given values into the above formula as follows.

                P = \frac{nRT}{V}

                   = \frac{0.725 mol \times 0.08206 Latm/mol K \times 294 K}{5.00 L}

                    = \frac{17.491089}{5} atm

                    = 3.498 atm

or,                = 3.50 atm (approx)

Therefore, we can conclude that the pressure of this mixture of gases is 3.50 atm.

4 0
3 years ago
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