Need some help -
PCl5 can be produced by the reaction of phosphorus trichloride with excess chlorine as follows: PCl3 + Cl2 → PCl5
If the actual yield is 127 g of PCl5 and the percent yield is 84.8%, what mass of PCl3 must be used? Hint: Use actual yield and percent yield to find theoretical yield and proceed from there.
a. 150 g
b. 98.8 g
c.108 g
d.83.8 g
e.71.1 g
2. If the reaction N2 + 3 H2 → 2 NH3 is carried out using 1.40 g of N2 and 0.400 g of H2, what mass of excess reactant will remain?
a. 0.200 g N2
b. 1.00 g N2
c. Both reactants will be completely consumed
d. 0.100 g H2
e.0.300 g H2
3. How many moles of bromine will react with 0.0500 mole of C2H2 in the reaction C2H4 + Br2 → C2H4Br2?
a. 0.186 mol
b. 2.00 mol
c. 0.0250 mol
d. 0.100 mol
e. 0.0500 mol
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Need some help - PCl5 can be produced by the reaction of phosphorus trichloride with excess...
Need some help - PCl5 can be produced by the reaction of phosphorus trichloride with excess chlorine as follows: PCl3 + Cl2 → PCl5 If the actual yield is 127 g of PCl5 and the percent yield is 84.8%, what mass of PCl3 must be used? Hint: Use actual yield and percent yield to find theoretical yield and proceed from there. a. 150 g b. 98.8 g c.108 g d.83.8 g e.71.1 g 2. If the reaction N2 + 3...
Please provide all steps and a detailed explanation 12. Phosphorus pentachloride can be produced by the reaction of phosphorus trichloride and chlorine gas. What mass of phosphorus trichloride must be used to produce 127 g of phosphorus pentachloride if the percent yield is 84.8%?
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