The molar mass of sulfur dioxide is 64,066 g.
SO3 has molecular mass (32x1+16x3)= 80.
So, 20g of SO3 is equal to 20/80 moles of SO3.
that is, equal to 0.25 moles of it.
20 g anhydrous sodium carbonate is equivalent to 0,188 moles.
molar mass Na2CO3 = 106 g/mol
20 g x 1 mol/106 g = 0.189 moles = 0.19 moles (to 2 significant figures)
0.625 moles of sulfur
Balanced equation. 2S + 3O2 --> 2SO3 1.32 moles O2 (2 moles SO3/3 moles O2) = 0.880 moles sulfur trioxide produced ========================
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
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.
2.24 L O2 (= 0.100 mol O2) is needed to react with 0.200 moles of SO2 to form SO3
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.
Balanced equation. 2S + 3O2 --> 2SO3 1.32 moles O2 (2 moles SO3/3 moles O2) = 0.880 moles sulfur trioxide produced ========================
There are 0.13 moles in 20 grams of magnesium nitrate.
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
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
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.
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
Moles = Mass/Molar Mass.Using this equation, we can take 25/(1.0 + 19) and find that it is equal to 1.25 moles.Keep in mind that very few significant figures were used for this example (2), and that if accuracy is to be expected, as many as possible should be used.
There are 6.023x10^23 molecules in one mole of a compound. So now, you have to find how many moles of each compound you have. CO's molecular weight is (12+16) = 28 g/mol N2's molecular weight is (14+14) = 28 g/mol So you find the moles of each. moles of N2 = 20g/ 28g/mol = .714 moles moles of CO = 16g / 28 g/mol = .571 moles So, N2 has (.714 *6.023x10^23) has 4.3 x10^23 molecules and CO (.571 *6.023x10^23) has 3.4x10^23 molecules. So, 20g of N2 has more molecules than 16g of CO