tungsten(VI) oxide reacts with hydrogen to produce tungsten metal and water. Wha
ID: 915562 • Letter: T
Question
tungsten(VI) oxide reacts with hydrogen to produce tungsten metal and water. What is the percent yield for the reaction if 4.00 g of tungsten (VI) oxide yield 2.80 g of tungsten metal.
A) Write the balanced equation. WO3+3H2--->3H2O+W is the balanced equation.
B) calculate the theoretical yield of Tungsten metal from the amount of starting material.
C) Calculate the percent yield foe the reaction.
D) if the reaction produces 900 J of heat, what is the molar heat of formation for tungsten metal?
Explanation / Answer
A) balanced equation : WO3 + 3H2 ---> 3H2O + W
B ) No of mole tungsten (VI) oxide = 4/231.84 = 0.01725 mol
sothat, if enough amount of H2 available.
No of mole of W produced = 0.01725 mol
Theoretical yield of W = 0.01725*183.84 = 3.17 grams
practicalyield = 2.8 grams
C ) percent yield = practicalyield/Theoretical yield*100
= 2.8/3.17*100 = 88.328%
D) Molar heat of formation of W (DHf0) = -900/0.01725 = -52.174 kj/mol
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