Assume that 8.5 L of iodine gas (I2) are produced at 0.75 atm and 295 K according to the following balanced equation: _ KI (aq) + _ Cl2 (g)→_ KCl (aq) + _ I2 (g)a. How many grams of KI were used?

we are given the pressure, volume and Temperature of the reaction. therefore we can used the ideal gas equation to determine the numner of mols of I₂ that formed

PV =nRT

n = PV/RT

= (0.75x 8.5)/(0.0821 x 295)

= 0.25 mols of I₂

we can see that the mole ratio between KI and I₂ is 2:1

therefore the number of mols of KI that must have reacted are

2/1 x 0.25 = 0.5 mols of KI

to find the mass we simply use

mass = mols x Molar mass

= 0.5 mols x 166.0g/mol

= 83 grams were used

Assume that 8.5 L of iodine gas (I2) are produced at 0.75 atm and 295 K according to the following balanced equation: ___ KI (aq) + ___ Cl2 (g)→___ KCl (aq) + ___ I2 (g)a. How many grams of KI were used?

Answer :

Other Questions

Assume that 8.5 L of iodine gas (I2) are produced at 0.75 atm and 295 K according to the following balanced equation: _ KI (aq) + _ Cl2 (g)→_ KCl (aq) + _ I2 (g)a. How many grams of KI were used?