What mass of phosphorus pentachloride would be produced by the complete reaction of 4.11 g of Cl2?
Answer:
Explanation:
A mole ratio is the ratio between the amounts in moles of any two compounds involved in a chemical reaction. The mole ratio can be determined by examining the coefficients in front of formulas in a balanced chemical equation.
Step 1: write the balanced chemical equation.
P4(s) + 10Cl2 (g) -----> 4PCl5(g)
Step 2: calculate the moles of Cl2
Moles of Cl2 = mass given / molar mass = ( 4.11 g / 70.906 g/mol ) = 0.058 mol
Step 3: Calculate the moles of phosphorus pentachloride
Sn(s) + 10Cl2 (g) -----> 4PCl5(s)
According to the reaction:
10 mol of Cl2 produces 4 mol of
PCl5
So, 0.058 mol of Cl2 will produced = ( 4 mol of PCl5 / 10 mol of Cl2 )× 0.058 mol of Cl2 = 0.0232 mol of PCl5
Step 4: Calculation of PCl5produced
we get moles of PCl5 that can be produced = 0.0232 mol
Mass of PCl5produced =( moles×molar mass ) = ( 0.0232 mol × 208.24 g/mol ) = 4.83 g
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chlorine according to the following reaction:
P4 (s) + 10 Cl2 (g) → 4
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Use the correct number of significant figures, fill in the
number ONLY!
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Please provide all steps and a detailed explanation
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