can you explain?
For each of the reactions shown, calculate how many grams of the product form when 16.8 g of the reactant in bold completely reacts. Assume that there is more than enough of the other reactant.
4 Cr(s) + 3 O2(g) 2 Cr2O3(s)
thanks
Sure! To calculate the number of grams of product that form when a given amount of reactant completely reacts, we need to use stoichiometry. Stoichiometry is a way of quantifying the relationship between the reactants and products in a chemical reaction.
In this case, we have the balanced equation:
4 Cr(s) + 3 O2(g) -> 2 Cr2O3(s)
To find the number of grams of Cr2O3 that form when 16.8 g of Cr(s) completely reacts, we can follow these steps:
1. Determine the molar mass of Cr(s).
- The molar mass of Cr(s) can be found from the periodic table. Cr has a molar mass of 52 g/mol.
2. Convert the given mass of Cr(s) to moles.
- We can use the equation: moles = mass / molar mass
- In this case, moles of Cr(s) = 16.8 g / 52 g/mol
3. Use the balanced equation to establish the stoichiometric ratio between Cr(s) and Cr2O3(s).
- From the equation, we can see that 4 moles of Cr(s) react to form 2 moles of Cr2O3(s).
4. Calculate the moles of Cr2O3(s) formed.
- We can use the stoichiometric ratio to convert moles of Cr(s) to moles of Cr2O3(s).
- Moles of Cr2O3(s) = (moles of Cr(s) / 4) * 2
5. Convert the moles of Cr2O3(s) to grams.
- We can use the equation: mass = moles * molar mass
- In this case, mass of Cr2O3(s) = moles of Cr2O3(s) * molar mass of Cr2O3(s)
By following these steps, you can calculate the number of grams of Cr2O3(s) that form when 16.8 g of Cr(s) completely reacts.