Question

In: Chemistry

9) for the reaction [ 2Al + 3H2SO4 → Al2(SO4)3 + 3 H2SO4] 6.0 g of...

9) for the reaction
[ 2Al + 3H2SO4 → Al2(SO4)3 + 3 H2SO4] 6.0 g of Al (MW=26.98 g/mol) are added to 12.0 mL of 0.20 M of H2SO4

A) what is the limiting reagent in the above reaction?

b) how many miles of H2SO4 will be formed?

c) how many grams of Al2(SO4)3 (MW=342.15 g/mol) are produced in the reaction?

Solutions

Expert Solution

2Al + 3H2SO4 → Al2(SO4)3 + 3 H2

no of moles of Al = W/G.A.Wt

                            = 6/26.98   = 0.2224 moles

no of moles of H2SO4 = molarity * volume in L

                                      = 0.2*0.012 = 0.0024 moles

2 moles of Al react with 3 moles of H2SO4

0.2224 moles of Al react with = 3*0.2224/2 = 0.3336 moles of H2SO4

H2SO4 is limiting reactant

3 moles of H2SO4 react with Al to gives 1 mole of Al2(SO4)3

0.3336 moles of H2So4 react with Al to gives = 1*0.3336/3 = 0.1112 moles of Al2(SO4)3

mass of Al2(So4)3 = no of moles* gram molar mass

                                = 0.1112*342.15   = 38.05 g >>>>answer

3 moles of H2SO4 react with Al to gives 3 moles of H2

0.3336 moles of H2SO4 react with Al to gives 0.3336 moles of H2

0.3336 moles of H2

  


Related Solutions

Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)?Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve...
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)?Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 14.7g . Part A What minimum mass of H2SO4 would you need? Express your answer in grams. Part B What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams.
Aluminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3(s)+3H2SO4(aq)→Al2(SO4)3(aq)+6H2O(l) 1)How many moles of Al2(SO4)3 can form...
Aluminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3(s)+3H2SO4(aq)→Al2(SO4)3(aq)+6H2O(l) 1)How many moles of Al2(SO4)3 can form under these conditions? 2)How many moles of the excess reactant remain after the completion of the reaction? Thank you!!
How many moles of Al2(SO4)3 are there in 10.26 g of Al2(SO4)3?
How many moles of Al2(SO4)3 are there in 10.26 g of Al2(SO4)3?
(a) The reaction of Al2(SO4)3 solution with NaOH forms a precipitate according to the equation: Al2(SO4)3...
(a) The reaction of Al2(SO4)3 solution with NaOH forms a precipitate according to the equation: Al2(SO4)3 (aq) + 6NAOH (aq) >>> 3Na2SO4 + 2Al(OH)3. (i) Which species is the precipitate? (b) The addition of more NaOH causes the precipitate in the initial reaction to redissolve: Al(OH)3 + NaOH >>> NaAl(OH)4 (aq) (ii) Write the formula of the complex ion. (iii) Write the net ionic equation for this reaction. (c) Finally, addition of an acid HCl to the solution in (b)...
In the following reaction2Al(s) + 3H2SO4(aq) -------Al2(SO4)3(aq) + 3H2(g) When 13.5 gram of Al is reacted...
In the following reaction2Al(s) + 3H2SO4(aq) -------Al2(SO4)3(aq) + 3H2(g) When 13.5 gram of Al is reacted with 3.00 M solution of H2SO4, whatvolume of solution is required to react with all of the Al?
Consider the following unbalanced equation for the reaction of aluminum with sulfuric acid. Al(s)+H2SO4(aq)→Al2(SO4)3(aq)+H2(g). How many...
Consider the following unbalanced equation for the reaction of aluminum with sulfuric acid. Al(s)+H2SO4(aq)→Al2(SO4)3(aq)+H2(g). How many moles of H2 are formed by the complete reaction of 0.384 mol of Al? Express your answer using three significant figures. Chemical Equation -> 2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g) Calculate the mass of water produced when 2.66 g of butane reacts with excess oxygen. Express your answer to three significant figures and include the appropriate units. Calculate the mass of butane needed to produce 62.7 g of carbon...
What is the TOTAL number of atoms in 10.26 g of Al2(SO4)3?
What is the TOTAL number of atoms in 10.26 g of Al2(SO4)3?
Determine the mass of oxygen in a 3.6 g sample of Al2(SO4)3. m(O) =
Determine the mass of oxygen in a 3.6 g sample of Al2(SO4)3. m(O) =
For the following reaction: 3H2SO4(g) + 2Fe(OH)3(s) → Fe2(SO4)3(s) + 6H2O(l) 1. Calculate ΔH°rx (in kJ)...
For the following reaction: 3H2SO4(g) + 2Fe(OH)3(s) → Fe2(SO4)3(s) + 6H2O(l) 1. Calculate ΔH°rx (in kJ) for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). 2. Calculate ΔS°rx (in J/K) for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 J/K). 3. Calculate ΔG°rx (in kJ) at 511.71 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and...
17.11 g of Al2(SO4)3 is dissolved in water to make 500 mL solution. What is the...
17.11 g of Al2(SO4)3 is dissolved in water to make 500 mL solution. What is the concentration of aluminum ion and sulfate ion in the resulting solution
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT