2Br- + Cl2 = 2Cl- +Br2 how many moles of chlorine gas, are required to react with 169g of bromide(Br-)?
Here is a sample of a stoichiometry problem.
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To find the number of moles of chlorine gas (Cl2) required to react with 169g of bromide (Br-), we need to use the concept of stoichiometry.
1. Start by determining the molar mass of bromide (Br-) and chlorine gas (Cl2).
- The molar mass of Br- is the molar mass of bromine minus one electron, which is approximately 79.9 g/mol (since the molar mass of bromine is 79.9 g/mol).
- The molar mass of Cl2 is the sum of two chlorine atoms, which is approximately 70.9 g/mol (since the molar mass of chlorine is 35.45 g/mol).
2. Next, calculate the number of moles of bromide (Br-) in 169g.
- Use the formula: Moles = Mass / Molar Mass
- Moles of Br- = 169g / 79.9 g/mol ≈ 2.11 moles of Br-
3. Based on the balanced chemical equation 2Br- + Cl2 = 2Cl- + Br2, we can see that the mole ratio between bromide (Br-) and chlorine gas (Cl2) is 1:1.
- This means that 2 moles of Br- will react with 1 mole of Cl2.
4. To determine the number of moles of Cl2 required, we can use the mole ratio from step 3.
- Moles of Cl2 = 2.11 moles of Br- × (1 mole Cl2 / 2 moles Br-) = 1.05 moles of Cl2
Therefore, approximately 1.05 moles of chlorine gas (Cl2) are required to react with 169g of bromide (Br-).