O 8/31/2016 11:55 PM A 80/100 8/31/2016 07:18 PM Gradebook Print Calculator Peri

Question

O 8/31/2016 11:55 PM A 80/100 8/31/2016 07:18 PM Gradebook Print Calculator Periodic Table x Incorrect X Incorrect Incorrect K Incorrect x Incorrect X Incorrect K Incorrect X x Question 28 of 30 ncorrect Map A General Chemistry 4th Edition University Science Books presented by Sapling Learning Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to How many milliliters of 3.50 M H2SO4(aq) are needed to react completely with 60.7 g of BaO2(s)? Number mL O Previous 3 Give Up & View Solution Check Answer Next SExit Hint

Explanation / Answer

First, identify how much BaO2 is there in mol

mol of BaO2 = mass of BaO2 / MW of BaO2

MW of BaO2 = 169.33 g of BaO2

mol of BaO2 = 60.7g / 169.33 g/mol = 0.3584 mol of BaO2

then

since the reaction is already balanced, the ratio is 1 mol of BaO2 per 1 mol of H2SO4

then

0.3584 mol of BaO2 = 0.3584 mol of H2SO4

We have concentation of H2SO4

M = mol/V

M = concentration

V = volume of solution in L

V = mol/M

V = 0.3584 /3.5 = 0.1024 L

but we need mL so

1 L = 1000 mL

0.1024 L = 0.1024*1000 = 102.4 mL of H2SO4 is required

Related Questions

Navigate

• Browse (All)
• Browse O
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.