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lilavasa [31]
3 years ago
12

How many grams of magnesium oxide forms when 8.0g of magnesium are burned?

Chemistry
1 answer:
AfilCa [17]3 years ago
7 0
Magnesium burns with oxygen to give magnesium oxide based on the following reaction:
2M<span>g</span>+<span>O<span>2 </span></span>........> 2Mg<span>O<span>(s)</span></span>+<span>energy
</span>From the periodic table:
molecular mass of magnesium = 24.3 grams
molecular mass of oxygen = 16 grams

From the reaction:
2 x 24.3 = 48.6 grams of magnesium are required to produce 2(24.3+16) = 80.6 grams of magnesium oxide.
We can know the amount of magnesium oxide produced from 8 grams of magnesium by simply doing cross multiplication as follows:
amount of magnesium oxide = (8 x 80.6) / 48.6 = 13.267 grams

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The atomic number identifies which of the following?
creativ13 [48]

Answer: protons

Explanation:

The atomic # identifies the amount of protons in an atom

4 0
2 years ago
A 0.175 M solution of an enantiomerically pure chiral compound D has an observed rotation of +0.27° in a 1-dm sample
-BARSIC- [3]

Answer:

The specific rotation of D is 11.60° mL/g dm

Explanation:

Given that:

The path length (l) =  1 dm

Observed rotation (∝) = + 0.27°

Molarity = 0.175 M

Molar mass = 133.0 g/mol

Concentration in (g/mL) = 0.175 mol/L × 133.0 g/mol

Concentration in (g/mL) = 23.275 g/L

Since 1 L = 1000 mL

Concentration in (g/mL) = 0.023275 g/mL

The specific rotation [∝] = ∝/(1×c)

= 0.27°/( 1  dm ×  0.023275 g/mL )

= 11.60° mL/g dm

Thus, the specific rotation of D is 11.60° mL/g dm

3 0
3 years ago
Which of the following is the correct name for MgCl2?
Studentka2010 [4]

Answer:

Magnesium dichloride

HoPe ThIs HeLpS! aNd HaVe A gOoD dAy!

8 0
2 years ago
A rigid container is filled with chlorine gas. The gas has a pressure of 2.75 bar. The tank is then cooled down to -20.0oC at wh
Gnom [1K]

Answer:

Original temperature (T1) = - 37.16°C

Explanation:

Given:

Gas pressure (P1) = 2.75 bar

Temperature (T2) = - 20°C

Gas pressure (P2) = 1.48 bar

Find:

Original temperature (T1)

Computation:

Using Gay-Lussac's Law

⇒ P1 / T1 = P2 / T2

⇒ 2.75 / T1 = 1.48 / (-20)

⇒ T1 = (2.75)(-20) / 1.48

⇒ T1 = -55 / 1.48

⇒ T1 = - 37.16°C

Original temperature (T1) = - 37.16°C

3 0
3 years ago
at 55 years what mass remains of a 200.0 g sample of a radioactive isotope with a half life of 10.0 years
Harman [31]

Answer:

4.419 g

Explanation:

     55 years is 5.5 half lives

200 g   *   (1/2)^5.5 = 4.419 g

3 0
1 year ago
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