According to the equation below, how many moles of NI3 are required to obtain exactly 0.5 moles of I2?2 NI3 ⟶⟶ N2 + 3 I2 0.17 mol 0.50 mol 0.33 mol 0.25 mol 1.0 mol
Question
According to the equation below, how many moles of NI3 are required to obtain exactly 0.5 moles of I2?2 NI3 ⟶⟶ N2 + 3 I2 0.17 mol 0.50 mol 0.33 mol 0.25 mol 1.0 mol
Solution
The balanced chemical equation is: 2 NI3 ⟶ N2 + 3 I2
This equation tells us that 2 moles of NI3 produce 3 moles of I2.
So, to find out how many moles of NI3 are needed to produce 0.5 moles of I2, we can set up a proportion:
(2 moles NI3 / 3 moles I2) = x moles NI3 / 0.5 moles I2
Solving for x gives us:
x = (2/3) * 0.5 = 0.33 moles NI3
So, 0.33 moles of NI3 are required to obtain exactly 0.5 moles of I2.
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