3 years ago

Arrhenius base definition

1 answer:

6 0

Arrhenius base is a substance that , when dissolved in an aqueous solution , increase the concentration of hydroxide (OH) ion in the solution

I hope that's help !

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What are atoms made up of

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They are made up of electrons, neutrons and protons

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The symbol for gold is a. go. b. g. c. au. d. au.

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Au is the symbol for gold. It comes from Latin word for gold, which is Aurunum. Its atomic number is 79.

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75.0 grams of MgCl, is dissolved in 500.0 g of water, density 1.00 g/ml. What is the MOLALITY of this solution?

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Octane (C8H18) is a component of gasoline that burns

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Calculate the mass of magnesium carbonate ( MgCO3), in grams, required to produce 110.0 g of carbon dioxide using the following

bearhunter [10]

Answer:

$210.7~g~MgCO_3$

Explanation:

We have to start with the reaction:

$MgCO_3~->~MgO~+~CO_2$

We have the same amount of atoms on both sides, so, we can continue. The next step is to find the number of moles that we have in the 110.0 g of carbon dioxide, to this, we have to know the atomic mass of each atom:

C: 12 g/mol

O: 16 g/mol

Mg: 23.3 g/mol

If we take into account the number of atoms in the formula, we can calculate the molar mass of carbon dioxide:

$(12*1)+(16*2)=44~g/mol$

In other words: $1~mol~CO_2=~44~g~CO_2$ . With this in mind, we can calculate the moles:

$110~g~CO_2\frac{1~mol~CO_2}{44~g~CO_2}=25~mol~CO_2$

Now, the molar ratio between carbon dioxide and magnesium carbonate is 1:1, so:

$2.5~mol~CO_2=2.5~mol~MgCO_3$

With the molar mass of $MgCO_3$ ( $(23.3*1)+(12*1)+(16*3)=84.3~g/mol$ . With this in mind, we can calculate the grams of magnesium carbonate:

$2.5~mol~MgCO_3\frac{84.3~g~MgCO_3}{1~mol~MgCO_3}=210.7~g~MgCO_3$

I hope it helps!

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3 years ago