How many grams of CH4 are needed to react with 160.0 grams of Br2
1. Write and balance the equation.
2. Convert 160 g bromine to moles. moles = grams/molar mass
3. Using the coefficients in the balanced equation convert moles Br2 to moles CH4.
4. Convert moles CH4 to grams. g = moles x molar mass.
To calculate the number of grams of CH4 needed to react with 160.0 grams of Br2, you need to use the concept of stoichiometry, which involves balancing the chemical equation, determining the molar ratio, and converting between moles and grams.
First, let's write the balanced chemical equation for the reaction between CH4 and Br2:
CH4 + Br2 -> CH3Br + HBr
The balanced equation tells us that one mole of CH4 reacts with one mole of Br2 to produce one mole of CH3Br and one mole of HBr.
Next, calculate the molar mass of CH4 and Br2:
- The molar mass of CH4 is 12.01 g/mol (carbon) + 4(1.008 g/mol) (hydrogen) = 16.04 g/mol.
- The molar mass of Br2 is 2(79.90 g/mol) = 159.80 g/mol.
Now, let's use the molar masses to convert the mass of Br2 to moles:
- Moles of Br2 = 160.0 g Br2 / 159.80 g/mol Br2 ≈ 1.0015 mol Br2
Since the balanced equation tells us that one mole of CH4 reacts with one mole of Br2, the moles of CH4 required will be the same as the moles of Br2.
Finally, convert the moles of CH4 to grams:
- Grams of CH4 = 1.0015 mol CH4 x 16.04 g/mol CH4 ≈ 16.07 g CH4
Therefore, approximately 16.07 grams of CH4 are needed to react with 160.0 grams of Br2.