1.) Enter your answer in the provided box
Calculate the mass % of O in barium periodate
? % O
2.) Be sure to answer all parts.
Write a balanced equation for the following by inserting the correct coefficients. If the coefficient equals 1, add "1" in the provided box.
??? CaSiO3(s) + ???? HF(g) → ??? CaF2(s) + ??? SiF4(g) + ???H2O(l)
3.) Be sure to answer all parts.
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen:
4KNO3(s) → 2K2O(s) + 2N2(g) + 5O2(g)
To produce 79.7 kg of O2, how many
(a) moles of KNO3 must be heated?
??mol
(b) grams of KNO3 must be heated?
??g
1.) molecular formula is Ba(IO4)2
molar mass = 519.13 g/mole
mass % of O in barium periodate = (8 * 16) * 100 / 519.13 = 23.66 %
2.) balanced equation is
1 CaSiO3(s) + 6 HF(g) ...............> 1 CaF2(s) + 1 SiF4(g) + 3 H2O(l)
3.) Be sure to answer all parts.
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen:
4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
4 mole KNO3(s) decompose 2 mole K2O(s) and 2 mole N2(g) and 5 mole O2(g).
79.7 kg of O2 = 79.7 * 1000 / 32 = 2490.6 mole.
(a) moles of KNO3 heated = (4 / 5) * 2490.6 = 1.66 * 10^3 mole.
(b) grams of KNO3 must be heated = 1.66 * 10^3 mole * 101.1032 g/mole = 167873 g = 1.68 * 10^5 g
1.) Enter your answer in the provided box Calculate the mass % of O in barium...
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