Considering the definition of molarity and molar mass, the mass of NaF required is 3.771 grams.
<h3>Definition of molarity</h3>Molar concentration or molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.
The molarity of a solution is calculated by dividing the moles of solute by the volume of the solution:
Molarity is expressed in units .
The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.
<h3 /><h3>Mass of NaF required</h3>In this case, you know:
Replacing in the definition of molarity:
Solving:
0.15 × 0.6 L= number of moles
<u><em>0.09 moles= number of moles</em></u>
The molar mass of NaF is 41. 9 g/mol. So, you can apply the following rule of three: If by definition of molar mass 1 mole of the compound contains 41.9 grams, 0.09 moles of the compound contains how much mass?
<u><em>mass= 3.771 grams</em></u>
Finally, the mass of NaF required is 3.771 grams.
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Answer:
0.145 moles de AlBr3.
Explanation:
¡Hola!
En este caso, al considerar la reacción química dada:
Al(s)+Br2(l)⟶AlBr3(s)
Es claro que primero debemos balancearla como se muestra a continuación:
2Al(s)+3Br2(l)⟶2AlBr3(s)
Así, calculamos las moles del producto AlBr3 por medio de las masas de ambos reactivos, con el fin de decidir el resultado correcto:
Así, inferimos que el valor correcto es 0.145 moles de AlBr3, dado que viene del reactivo límite que es el aluminio.
¡Saludos!