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viva [34]
3 years ago
8

What volume of 0.05 mol/L HCl is required to react with 5.00g of manganese dioxide according to this equation?

Chemistry
1 answer:
adell [148]3 years ago
4 0

217 ml of 0.05 M HCl will be required to react with 5 gm of MnO2 according to the equation given.

Explanation:

The balanced chemical equation is given as:

4HCl(aq) + MnO2(s) → 2H2O(l) + MnCl2(aq) + Cl2(g)

This shows that 4 moles of HCl reacts with 1 mole of MnO2

the mass of Manganese oxide is given as 5 grams

molar mass of MnO2 = 86.93 grams/mole

number of moles of MnO2 is given by

number of moles = \frac{mass}{atomic mass of one mole}

number of moles= \frac{5}{86.93}

                            = 0.0575 moles of MnO2

From the equation:

4 moles of HCl reacts with 1 mole of MnO2

x moles of HCl reacts with \frac{0.0575}{x} moles of MnO2

\frac{1}{4} = \frac{0.0575}{x}

= 0.23 moles of HCl will react

atomic mass of HCl = 36.46 Grams/mole

mass = 0.23 x 36.46

         = 8.3858 grams.of HCl

molarity of HCl = \frac{number of moles}{volume in liters}

volume is 1 litre

so molarity is 0.23 M

Using the formula

M1V1 = M2V2

0.05 x 1 = 0.23 X x

x = 0.217 litre

so 217 ml of 0.05 M HCl will be required to react with 5 gm of MnO2.

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Se hace reaccionar 4,00 g de aluminio y 42,00 g de bromo, según la reacción: Al(s)+Br2(l)⟶AlBr3(s) Calcular las moles de AlBr3(s
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Explanation:

¡Hola!

En este caso, al considerar la reacción química dada:

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Es claro que primero debemos balancearla como se muestra a continuación:

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Así, calculamos las moles del producto AlBr3 por medio de las masas de ambos reactivos, con el fin de decidir el resultado correcto:

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Así, inferimos que el valor correcto es 0.145 moles de AlBr3, dado que viene del reactivo límite que es el aluminio.

¡Saludos!

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