PLEASE show how to convert to moles and then tell the limiting reactant.
We have 0.316 grams of p-anisaldehyde and 0.25mL of acetophenone.
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PLEASE show how to convert to moles and then tell the limiting reactant. We have 0.316...
Find the limiting reactant of the experiment by converting reactants to product (remember to show all calculations used) Calculate the theoretical yield Calculate the percent yield using the limiting reactant data: melting point of trans P-anisalacetophenone: 73.0-76.0 C Density pf P-anisalahyde: 1.1191g/cm^3 Density of acetophenone: 1.0281g/gcm^3 Molar mass of trans P- anisalacetophenone: 238.28g/mol Molar mass of P-anisaldehyde: 136.15g/mol Molar mass of acetophenone: 120.15g/mol P-anisalaehyde used: 1.03ml Acetophenone used: 1.06ml 3.0ml ethanol first recrystallization 6 drops of sodium hydroxide 15ml of...
6)# What is the limiting reactant for the following reaction given we have 3.4 moles of Ca(NO3)2 and 2.4 moles of Li3PO4? Reaction: 3Ca(NO3)2 + 2Li3PO4 ---> 6LiNO3 + Ca3(PO4)2 Answer (show work please?) Ca3(PO4)2 Li3PO4 Ca(NO3)2 LiNO3 not enough information
What is the limiting reactant for the following reaction given we have 1.3 moles of HCl and 0.7 moles of Ca(OH)2? Reaction: 2HCl + Ca(OH)2 → 2H2O + CaCl2 (a) Ca(OH)2 (b) CaCl2 (c) H2O (d) HCl
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the balanced chemical equation. Use mole ratio, then convert to grams. A method used by the EPA for determining the ozone concentration in the air is to pass an air sample through a bubbler containing iodide ions. The iodide ions remove the ozone according to the following reaction: O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(aq) + 2 OH-(aq) How many grams of ozone...
which reactant is limiting? which reactant is in excess? actual yield of NaCl, show the calculation percent yield of NaCl, show calculation Data 50.00 g Mass of beaker: Mass of beaker and sample (NaHCO3): Mass of sample (NaHCO3): s1.00 g 49.57 g 49.57 g Mass of beaker and residue first heating: Mass of beaker and residue second heating: Mass of beaker and residue third heating (if required): Mass of residue: g 0.43 g mL Volume of concentrated HCl added: Calculations...
Solving moles-to-moles limiting reactant problems Nitrogen (N2) gas and hydrogen (H) gas react to form ammonia (NH) gas. Suppose you have 9.0 mol of N, and 1.0 mol of H, in a reactor. What would be the limiting reactant? Enter its chemical formula below.
STUDY GUIDE - MOLES Here to determine how much Xeo, forms, simply convert the 0.0412 mol Xeos the XeF. reacting, into grams: 0.0412 mol Xerox 1708XO - 7.37 g Xeos 7) The amount of the excess reactant, water, reacted can be calculated from 0.0412 mol XeF: 12 mol Xco, formed by all of The remaining excess water is be calculated from the limiting reactant, 0.0412 mel Xerx 3 mol H20 18.02 -221 H2O (reacted) 1 mol Xer, * 1 molde...
If 58 moles of NH3 are combined with 32 moles of sulfuric acid, what is the limiting reactant and how much of the excess reactant is left over? 2 NH3 + H2SO4 (NH4)2SO4 A) H2SO4, 29 mol B) NH3, 1.0 mol C) NH3 29 mol D) NH3, 3.0 mol E) H2SO4, 3.0 mol
EXPERIMENT # 14 Assuming Na2CO, is the limiting reactant, how many grams of NaCl can be produced from the amount of Na2CO, used in this experiment? Show calculations below: 8 Assuming HCI is the limiting reactant, how many gran of NaCl can be produced from the amount of HCI user this experiment? Show calculations below: 8 Which reactant is limiting? Which reactant is excess? 8 Actual yield of NaCl 8 Theoretical yield of NaCl % Percent yield of NaCl Show...
Considering the limiting reactant concept, how many moles of C are produced from the reaction of 2.00 mole A and 4.50 mole B? A(g) + 3B(g) -----> 2C(g)