Problemas
1.)If you fully react 23.grams of S. how much Li_(2)S would you produce from the reaction? 1S_(0)+16Liarrow 8Li_(2)S
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Respuesta
To solve this problem, we need to use the balanced chemical equation and the given information to determine the amount of
produced.Given information:- The balanced chemical equation is:
- The amount of
reacted is 23 grams.Step 1: Calculate the molar mass of
.The molar mass of
is 32.06 g/mol.Step 2: Calculate the number of moles of
reacted.Number of moles of
= Mass of
/ Molar mass of
Number of moles of
= 23 g / 32.06 g/mol = 0.714 molStep 3: Use the balanced chemical equation to determine the number of moles of
produced.According to the balanced equation, 1 mole of
produces 8 moles of
.Number of moles of
produced = 0.714 mol × 8 = 5.712 molStep 4: Calculate the molar mass of
.The molar mass of
is 45.92 g/mol.Step 5: Calculate the mass of
produced.Mass of
= Number of moles of
× Molar mass of
Mass of
= 5.712 mol × 45.92 g/mol = 261.6 gTherefore, if you fully react 23 grams of
, you would produce 261.6 grams of
from the reaction.