Please help me!!!
For the reaction, calculate how many grams of the product form when 3.0 g of Cl2 completely reacts.
Assume that there is more than enough of the other reactant.
2Na(s)+Cl2(g)→2NaCl(s)
Same type problem.
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To calculate the number of grams of the product that form when a certain amount of a reactant is completely consumed in a chemical reaction, you need to use stoichiometry.
First, let's identify the balanced equation for the reaction:
2 Na(s) + Cl2(g) → 2 NaCl(s)
From the balanced equation, we can see that for every 1 mole of Cl2 that reacts, 2 moles of NaCl are formed.
Step 1: Convert grams of Cl2 to moles.
To do this, we need to know the molar mass of Cl2, which is approximately 70.906 g/mol (you can find this value on the periodic table).
Using the molar mass, we can calculate the number of moles of Cl2:
moles of Cl2 = mass of Cl2 / molar mass of Cl2
moles of Cl2 = 3.0 g / 70.906 g/mol
Step 2: Use the stoichiometry of the balanced equation to determine the moles of NaCl formed.
From the balanced equation, we know that 2 moles of NaCl are formed for every 1 mole of Cl2 that reacts.
moles of NaCl = moles of Cl2 × (2 moles NaCl / 1 mole Cl2)
Step 3: Convert moles of NaCl to grams.
To do this, you need to know the molar mass of NaCl, which is approximately 58.443 g/mol. Using the molar mass, we can calculate the mass of NaCl:
mass of NaCl = moles of NaCl × molar mass of NaCl
By plugging in the numbers from the previous steps, you can calculate the final answer:
mass of NaCl = (moles of Cl2 × (2 moles NaCl / 1 mole Cl2)) × molar mass of NaCl