The following reaction is used to produce tungsten(VI)oxide: WS3(s) + O2(g) �¨ WO3(s) + SO2(g)
The WO3 is then heated and undergoes a decomposition reaction produce tungsten and oxygen gas. How many grams of tungsten could be produced if 39.27 grams of WS3 are used
You should first balance the equation given.
WS3(s) + O2(g) -> WO3(s) + SO2(g)
But you should see that one mole of WS3 must yield one mole of WO3.
You also have the decomposition of WO3
WO3 -> W + O2
Again one mole of WO3 yields one mole of W metal.
So calculate the number of moles of WS3 you are starting with from
39.27/(molar mass of WS3)
this is the same number of moles of W metal produced so mass produced
39.27x(molar mass of W)/(molar mass of WS3)
To find out how many grams of tungsten could be produced, we first need to determine the molar mass of WS3 and tungsten (W).
1. Calculate the molar mass of WS3:
W = 183.84 g/mol
S = 32.06 g/mol
The molar mass of WS3 is: (1 * 183.84) + (3 * 32.06) = 280.02 g/mol
2. Convert the given mass of WS3 to moles:
Moles = Mass / Molar mass
Moles = 39.27 g / 280.02 g/mol
Moles = 0.14 mol
3. Use the balanced equation to determine the stoichiometric ratio between WS3 and W:
WS3(s) + O2(g) → WO3(s) + SO2(g)
Balanced equation: 2 WS3 → 2 W + 3 SO2
From the balanced equation, we can see that it takes 2 moles of WS3 to produce 2 moles of W.
4. Convert moles of WS3 to moles of W using the stoichiometric ratio:
Moles of W = Moles of WS3 * (2 moles of W / 2 Moles of WS3)
Moles of W = 0.14 mol * (2 / 2)
Moles of W = 0.14 mol
5. Convert moles of W to grams using the molar mass of tungsten:
Mass of W = Moles of W * Molar mass of W
Mass of W = 0.14 mol * 183.84 g/mol
Mass of W = 25.75 g
Therefore, if 39.27 grams of WS3 are used, approximately 25.75 grams of tungsten could be produced.