Balanced equation.
2S + 3O2 --> 2SO3
1.32 moles O2 (2 moles SO3/3 moles O2)
= 0.880 moles sulfur trioxide produced
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The molar mass of sulfur dioxide is 64,066 g.
2S + 3O2 >> 2SO3 8.0 grams O2 (1 mole O2/32 grams)(2 mole SO3/3 mole O2) = 0.1666 ( 0.17 moles SO3 ) and also, 0.1666 moles SO3 (80.07 grams/1 mole SO3) = 13.34 ( 13 grams SO3 ) if needed.
Since oxygen is diatomic it requires 2 moles of oxygen.
molar mass SO3 = 80 g/mole. 1.12 moles x 80 g/mole = 89.6 grams
2.24 L O2 (= 0.100 mol O2) is needed to react with 0.200 moles of SO2 to form SO3
First you need to find the balanced reaction:2S + 3O2 --> 2SO3So using the balanced reaction we see that for every 3 moles of oxygen consumed, 2 moles of sulfur trioxide are produced:1.2 moles O2 consumed * (2 moles SO3/3 moles O2) = 0.8 mole of SO3 produced
The most straightforward reaction for the formation of SO3 from SO2 is 2 SO2 + O2 => 2 SO3. If this is the actual reaction for the formation, 3 moles of SO3 are formed from 3 moles of SO2.
The molar mass of sulfur dioxide is 64,066 g.
2S + 3O2 >> 2SO3 8.0 grams O2 (1 mole O2/32 grams)(2 mole SO3/3 mole O2) = 0.1666 ( 0.17 moles SO3 ) and also, 0.1666 moles SO3 (80.07 grams/1 mole SO3) = 13.34 ( 13 grams SO3 ) if needed.
Since oxygen is diatomic it requires 2 moles of oxygen.
molar mass SO3 = 80 g/mole. 1.12 moles x 80 g/mole = 89.6 grams
I assume you mean atoms. 2.4 X 10^24 atoms SO3 ( 1mol SO3/6.022 X 10^23 ) = 3.985 mol
2.24 L O2 (= 0.100 mol O2) is needed to react with 0.200 moles of SO2 to form SO3
Simply divide by the number that signifies moles of any thing; Avogadro's number. 3.4 X 10^23/6.022 X 10^23 = 0.56 moles of H2SO4
Molar mass of (NH4)2SO4 is 132.14 g/mol, so4.69 (g) / 132.14 (g/mol) = 0.0355 mol
i bet its 2.0g
The compound Sn SO3 2 is Tin (IV) Sulphite. It can be produced easily in a chemistry lab, but has few if any commercial applications.