In given compounds, thereare 1Na, 1Al, 2S, 8O, 24H and 12O.
Therefore, formula mass of NaAl(SO4)2.12H2O
= Molar mass of (1Na + 1Al + 2S + 20O + 24H )
= 22.98 g/m + 26.98 g/m + ( 2 x 32 g/m) + ( 20 x 16 g/m )
+ (24 x 1 g/mol )
= 22.98 g/m + 26.98 g/m + 64 g/m + 320 g/m + 24 g/m
= 457.96g/m.
Ans = Formula mass = 457.96 g/mole.
muy 2A Lab 12: Synthesis of Alum 1. Calculate the formula mass of NaAl(SO4)2 12H20. 2. Calculate the moles of 1.00 gram aluminum. 3. Using the answer from question 2, calculate the moles of NaAl(SO4)2 12H20 that can be produced given the following balanced chemical equation: Nat! + A1*3 + 28042 +12H20 → NaAl(SO4)2 12H20 4. Calculate the grams of NaAl(SO4)2 12H2O from the answer in question 3. 5. If 14.34 g of NaAl(SO4)2 12H20 was produced from the reaction,...
Calculate the molar mass of alum, KAI(SO4)2·12H20 (potassium aluminum sulfate dodecahydrate). Type the molar mass without units, to the nearest whole number.
Prelab Questions: Name 1) What is the molar mass of KAl(SO4)2 12H20 ? (the 12 waters are part of the molecule) 2) Calculate the mass of alum that can be produced from 14.471g of Al 3) Calculate the mass of alum that can be formed from 0.724 moles of KOH 4) Calculate the mass of alum that can be formed from 1.10 mole of H2SO4 5) a) Based on the data above which reactant is the limiting reactant? b) What...
i Supporting calculations: The net reaction is: 2Al(s) + 2KOH + 22H20 + 4H2SO4 → 2KAI(SO4)2:12H20 + 3H2 Theoretical yield of alum 1.01g| I mol All2 mol KAl(SO4)2 #12 H2O1 26.989 Al 2 mol Al 1 mol KAI(SO4)2:12H20
ed chemical equation. However, the balanced chemical equation only works in units of moles. To convert grams of aluminum to moles of aluminum the atomic mass of aluminum must be used. grams of aluminum x 1 mole Al = 1 26.98 g Al To relate the moles of aluminum to KAl(SO4)2* 12H20, the mole to mole ratio must be found in the balanced chemical equation. In this case it is: 1 mole of Al3 = 1 mole KAl(SO4)2 12H20 As...
(12) 2. The chemical formula for cupric phosphate is Fe (SO4)3. Determine the following: a. the number of atoms in two formula units of Fe2(SO4)3 b. the number of sulfur atoms in 1.75 mole of Fe2(SO4)3 c. the mass in grams of 2.65 mol of Fe2(SO4)3 d. the number of moles of Fe2(SO4)3 in 3.45 grams of Fe2(SO4)3 e, the mass in grams of 3 formula units of Fe2(SO4),
Determine the reactions occurring in the following equations 1) Al2(SO4)3(aq) + K2SO4(aq) + 24 H2O(l) ----> 2KAl(SO4)2 * 12H2O(s) 2) 2Al(s) + 2KOH(aq) +4 H2SO4(aq) + 22H20(l) - - - > 2KAl(SO4)2*12H20(s) + 3H2(g) The following is a bank for the types of reactions that can be occurring. Two or more can be present in one equation. Metathesis Reactions Redox Reactions Single Displacement Reactions Double Displacement Reactions Combination Reactions Decomposition Reactions
1. Calculate the formula mass for BaSO4 2. What is the percent by mass of oxygen in sodium nitrate?
percent error #3 Calculations for Part 2 Ou in KAl(SO4)2 1. Experimental value for percent sulfate in alum BA 0.15793504) H20 12 ( 18.0a)= 216.24 KAYS0y), 12H20 MM (504)₂ = 64.327 128.00 2 = 192.32 glmor 2. Theoretical value for percent sulfate in alum are monologa dobar odbud 3. Percent error Results and Data Analysis Table 1: Determination of the Water of Hydration in Alum Crystals Mass of crucible + cover + alum 43.10509 - water Mass of crucible +...
HULIOL QUESTION 7 The formula for ammonium sulfate is a. NH4(SO4)2 b. NH4504 c. (NH4)2(SO4)2 d. (NH4)2SO4