Determine the theoretical yield if 0.5 moles of zinc is used to form ZnI2 ___ Zn...
Determine the theoretical yield if 0.5 moles of zinc is used to form ZnI2
___ Zn + __I2 → ___ZnI2
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Determine the theoretical yield if 0.5 moles of zinc is used to
form ZnI2
___ Zn...
Write a balanced equation for the combination of zinc and iodine to form zinc iodide, ZnI2....
Write a balanced equation for the combination of zinc and iodine to form zinc iodide, ZnI2. Phase symbols are not graded. balanced equation: Zn +1 — Znl, How many moles of zinc are required to react with four moles of iodine? moles of zinc: mol zinc
1. Calculate the theoretical yield of based on Equation 1 and the initial mass of the...
1. Calculate the theoretical yield of
based on Equation 1 and the initial mass of the limiting
reagent.
Equation (1) Zn(s) + I2(s) → ZnI2(s)
Mass of Zinc 0.6404 g
Mass of Iodine 0.6544 g
Mass of dried Zinc Iodide (Experimental Yield) 0.6986 g
How many moles of zinc, Zn , are in 1.37 × 10 24 Zn atoms?
How many moles of zinc, Zn , are in 1.37 × 10 24 Zn atoms?
Chem 143 - Lab 46) CALCULATE THE THEORETICAL YIELD Grams of sodium carbonate used Moles of...
Chem 143 - Lab 46) CALCULATE THE THEORETICAL YIELD Grams of sodium carbonate used Moles of sodium carbonate used Grams of calcium chloride used Moles of calcium chloride used Moles of precipitate expected Theoretical yield of precipitate in grams Actual yield of precipitate in grams Percent yield 5.6 Show detailed work for percent yield. Page 4 of 4 Chem 143 - Lab Pre-lab Exercise Show the details of each calculation to get full credit 1. Magnesium oxide, a white powdery...
First determine the actual yield, moles of Sr3(PO4)2 formed. From the actual yield, theoretical moles of...
First determine the actual yield, moles of Sr3(PO4)2 formed. From the actual yield, theoretical moles of limiting reactant in sample: a) Theoretical mass of limiting reactant b) Mass percent of limiting reactant in sample From the actual yield, mass of excess reactant sample, what is the mass percent of excess in sample? Beaker Sample II Unknown mixture NaPO412H2O * SrCl2* 6H2O Mass of mixture and container 113.4904g Mass of container 111.5575g Mass of mixture added to Beaker II 1.9329g Formula...
1. Zinc nitrate reacts with potassium phosphate to form the insoluble compound, zinc phosphate. The reaction...
1. Zinc nitrate reacts with potassium phosphate to form the insoluble compound, zinc phosphate. The reaction proceeds according to the balanced equation below: 3 Zn(NO3)2 (aq) + 2 K3PO4 (aq) → Zn3(PO4)2 (s) + 6 KNO3 (aq) A mass of 0.1420 g is desired as the yield of zinc phosphate. Calculate the moles of desired product. 2. 2 Al(NO3)3 (aq) + 3 K2Cr2O7 (aq) → Al2(Cr2O7)3 (s) + 6 KNO3 (aq) Aluminum nitrate reacts with potassium dichromate to form the...
Determination of theoretical yield NaCl: volume HCl used (L) molarity HCl (mol/L) moles HCl available to...
Determination of theoretical yield NaCl: volume HCl used (L) molarity HCl (mol/L) moles HCl available to react Type answer here 1.998 volume NaOH used (L) molarity NaOH (mol/L) 2.016 moles NaOH available to react Type answer here Theoretical yield of NaCl, expressed as moles NaCl: Type answer here
Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. 4 Zn(s) +...
Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. 4 Zn(s) + 10 HNO3(aq) - 4 Zn(NO3)2(aq) + NH4NO3(aq)+ 3 H20(0) (a) How many atoms of zinc react with 1.05 g HNO3? atoms (b) Calculate the number of grams of zinc that must react with an excess of HNO3 to form 28.3g NH4NO3
According to the following reaction, how many moles of zinc hydroxide are necessary to form 0.908 moles zinc sulfate? s...
According to the following reaction, how many moles of zinc hydroxide are necessary to form 0.908 moles zinc sulfate? sulfuric acid (aq) + zinc hydroxide (s) = zinc sulfate (aq) + water (l) Nitrogen monoxide is produced by combustion in an automobile engine. According to the following reaction, how many moles of oxygen gas are necessary to form 0.230 moles nitrogen dioxide? nitrogen monoxide (g) + oxygen (g) = nitrogen dioxide (g) According to the following reaction, how many moles...
Question 6 (2 points) Determine the theoretical yield of HCl (in moles) if 0.50 mol of...
Question 6 (2 points) Determine the theoretical yield of HCl (in moles) if 0.50 mol of BCl3 and 2.1 mol of H20 are reacted according to the following balanced reaction. BC13(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g) O 1.5 mol O2.1 mol 0 0.70 0 0.17 O 0.5 Question 7 (2 points) Determine the quantity of excess reactant (in moles) that remains after a reaction if 0.50 mol of BCl3 and 2.1 mol of H20 are reacted according...
Write a balanced equation for the combination of zinc and iodine to form zinc iodide, ZnI2. Phase symbols are not graded. balanced equation: Zn +1 — Znl, How many moles of zinc are required to react with four moles of iodine? moles of zinc: mol zinc
1. Calculate the theoretical yield of
based on Equation 1 and the initial mass of the limiting
reagent.
Equation (1) Zn(s) + I2(s) → ZnI2(s)
Mass of Zinc 0.6404 g
Mass of Iodine 0.6544 g
Mass of dried Zinc Iodide (Experimental Yield) 0.6986 g
Chem 143 - Lab 46) CALCULATE THE THEORETICAL YIELD Grams of sodium carbonate used Moles of sodium carbonate used Grams of calcium chloride used Moles of calcium chloride used Moles of precipitate expected Theoretical yield of precipitate in grams Actual yield of precipitate in grams Percent yield 5.6 Show detailed work for percent yield. Page 4 of 4 Chem 143 - Lab Pre-lab Exercise Show the details of each calculation to get full credit 1. Magnesium oxide, a white powdery...
Determination of theoretical yield NaCl: volume HCl used (L) molarity HCl (mol/L) moles HCl available to react Type answer here 1.998 volume NaOH used (L) molarity NaOH (mol/L) 2.016 moles NaOH available to react Type answer here Theoretical yield of NaCl, expressed as moles NaCl: Type answer here
Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. 4 Zn(s) + 10 HNO3(aq) - 4 Zn(NO3)2(aq) + NH4NO3(aq)+ 3 H20(0) (a) How many atoms of zinc react with 1.05 g HNO3? atoms (b) Calculate the number of grams of zinc that must react with an excess of HNO3 to form 28.3g NH4NO3
Question 6 (2 points) Determine the theoretical yield of HCl (in moles) if 0.50 mol of BCl3 and 2.1 mol of H20 are reacted according to the following balanced reaction. BC13(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g) O 1.5 mol O2.1 mol 0 0.70 0 0.17 O 0.5 Question 7 (2 points) Determine the quantity of excess reactant (in moles) that remains after a reaction if 0.50 mol of BCl3 and 2.1 mol of H20 are reacted according...
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