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2 years ago

Dana wants to determine the molar mass of magnesium hydroxide, Mg(OH)2. Which calculation should she use?

Chemistry

2 answers:

AVprozaik [17]2 years ago

7 0

Answer:

C is correct

Explanation:

The molar mass is the total mass of a compound, that means, you need to add the mass of every single atom in the formula. In this case, you have one atom of Magnesium, two atoms of Oxygen and two atoms of Hydrogen, that is the reason why you need to multiply molar mass x 2 in the case of Oxygen and Hydrogen

aleksandr82 [10.1K]2 years ago

3 0

Answer C. is correct:

(molar mass of Mg) + (2 x molar mass of O) + (2 x molar mass of H)

:-) ;-)

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Where were atoms formed ?

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Answer:

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3 years ago

What is typically displayed on the y-axis of a solubility curve?

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3 years ago

Consider the reaction Mg₂Si(s) + 4 H₂O(ℓ) → 2 Mg(OH)₂(aq) + SiH₄(g). How many grams of silane gas (SiH₄) are formed if 25.0 g of

Neko [114]

Answer:

10.60 grams of silane gas are formed.

Explanation:

From the reaction:

Mg₂Si(s) + 4H₂O(l) → 2Mg(OH)₂(aq) + SiH₄(g)

We know that the limiting reactant is Mg₂Si, so to find the mass of SiH₄ formed we need to calculate the number of moles of Mg₂Si:

$\eta_{Mg_{2}Si} = \frac{m_{Mg_{2}Si}}{M_{Mg_{2}Si}}$

Where:

m: is the mass of Mg₂Si = 25.0 g

M: is the molar mass of Mg₂Si = 76.69 g/mol

$\eta_{Mg_{2}Si} = \frac{m_{Mg_{2}Si}}{M_{Mg_{2}Si}} = \frac{25.0 g}{76.69 g/mol} = 0.33 moles$

Now, the stoichiometric relation between Mg₂Si and SiH₄ is 1:1 so:

$\eta_{Mg_{2}Si} = \eta_{SiH_{4}} = 0.33 moles$

Finally, the mass of SiH₄ is:

$m_{SiH_{4}} = \eta_{SiH_{4}}*M_{SiH_{4}} = 0.33 moles*32.12 g/mol = 10.60 g$

Therefore, 10.60 grams of silane gas are formed.

I hope it helps you!

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3 years ago

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3 years ago

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Anvisha [2.4K]

Answer:

Explanation:

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2,5

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