How many millliters of 2.75 M #H_2SO_4(aq)# are needed to react completely with 47.5 g of #BaO_2(s)#?

Question

Naomi Aronson · Accepted Answer

# 102 \ mL#

Write a balanced chemical equation for the reaction between barium peroxide and sulfuric acid.

#BaO_2 + H_2SO_4 -> BaSO_4 + H_2O_2#

Use the stoichiometry of the equation to find the number of moles of sulfuric acid reacted.

#47.5 \ g \ BaO_2xx (1 mol. BaO_2)/(169.33 \ g \ BaO_2)xx (1\ mol. H_2SO_4)/(1\ mol.\ BaO_2)#

#47.5 cancel(\ g \ BaO_2)xx (1 color(red)cancel(\ mol. BaO_2))/(169.33 cancel(\ g \ BaO_2))xx (1\ mol. H_2SO_4)/(1color(red)cancel(\ mol.\ BaO_2))#

#0.281 \ mol.\ H_2SO_4#

Now, use the molarity formula to find the volume of the sulfuric acid used.

#C_M = n/ V#

Where:

#C_M " "# is the molarity of the acid solution expressed in mol/L.

#V " "# is the volume of the acid solution expressed L.

# n" "# is the number of moles.

#V = n / C_M#

#V = ( 0.281 \ mol.)/(2.75 \ mol. L^-1)#

#V = 0.102 \ L#

#V = 102 \ mL#

Peyton Adams · Answer

undefined Determine the moles of BaO2 and H2SO4 by using the mole ratio. Then, convert the results to milliliters. The moles of BaO2 are 0.369 mol, the moles of H2SO4 are 1.108 mol, and the needed milliliters of 2.75 M H2SO4 are 403 mL.