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ivolga24 [154]
3 years ago
12

Balancing oxidation-reduction reactions Mg+ N2—>Mg3N2

Chemistry
1 answer:
BartSMP [9]3 years ago
3 0

Answer:

{ \sf{3Mg_{(s)} + N_{2(g)} →Mg _{3}N_{2(s)}}}

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Melted rock can ooze out from below earths surface through a crack in the crust called a(n)?
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Melted rock can ooze out from below the earth's surface through a crack called a fault.
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3 years ago
Determine the concentration of an HBr solution if a 45.00 mL aliquot of the solution yields 0.5555 g AgBr when added to a soluti
amid [387]
Molecular weight of AgBr = 187.7
moles of Ag = \frac{0.5555}{187.7} = 2.96 x 10^{-3}
moles of Br = moles of Ag = 2.96 x 10⁻³ mol
concentration of HBr (Molarity) = conc. of Br (strong acid) = \frac{2.96 x 10^{-3} }{45 x 10^{-3} } = 0.0658 mol/l
6 0
2 years ago
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List earth and the gas giant planets from the hottest to the coldest planet
inessss [21]

Answer:

1. Venus

471°C

2. Mercury

(430°C) during the day,  (-180°C) at night

3. Earth

16°C

4. Mars

-28°C

5. Jupiter

-108°C

6. Saturn

-138°C

7. Uranus

-195°C

8. Neptune

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Explanation:

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8 0
2 years ago
What mass of hbr (in g) would you need to dissolve a 3.4 −g pure iron bar on a padlock?
vivado [14]

<u>Given:</u>

Mass of pure iron (Fe) = 3.4 g

<u>To determine:</u>

Mass of HBr needed to dissolve the above iron

<u>Explanation:</u>

Reaction between HBr and Fe is

Fe + 2HBr → FeBr₂ + H₂

Based on the reaction stoichiometry-

1 mole of Fe reacts with 2 moles of HBr

# moles of Fe = mass of Fe/atomic mass of Fe = 3.4/56 g.mol⁻¹ = 0.0607 moles

Therefore # moles of HBr = 2*0.0607 = 0.1214 moles

Molar mass of HBr = 81 g/mole

Mass of HBr = 0.1214 moles * 81 g/mole = 9.83 g

Ans: Mass of HBR required is 9.83 g

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3 years ago
Methyl phenolphthalein and litmus
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Both are the indicators which helps to identity the acid and base

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3 years ago
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