using the following information: masses; 125ml flask=63.46ml; 100ml beaker=31.80

Question

using the following information: masses; 125ml flask=63.46ml; 100ml beaker=31.80ml; zinc=2.0g; iodine=2.0g; flask & zinc=64.85ml; beaker & product=34.46ml

1. calculate the total mass of zinc and iodine before the reaction (show/lable calculations)

2. calculate the % difference between the mass of the product and the sum of the masses of reactants (using the following formuala) % difference=(mass of product) - (sum of the masses of the reactants)/sum of the masses of reactants X 100%

3. calculate the following: a) total mass of the excess zinc and zinc iodinde after the reaction b) the number of moles of iodine consumed in the reaction c)the number of moles of zinc consumed in the reaction

Explanation / Answer

Q1.

mass of zin = 2 g

mass of iozine = 2

total mass = 2+2 = 4 g

Q2.

% diff. between mass of product and sum of reactants...

NOTE: assume the units are acutaly "MASS" and not "mL"

so..

mass of products = 34.46-31.80 = 2.66 g

change = 2.66-2 = 0.66 g extra

% change = 0.66/2 *100 = 33%

Q3

mol of Iodine = mass/MW = 2/253.808940 = 0.0078799

mol of Zn = mass/MW = 2/65.38 = 0.03059

ratio is:

Zn + I2 = ZnI2

so

1:1

I2 limits

0.0078799 mol of I2 react to form 0.0078799 mol of ZnI2

mol of Zn reacts = 0.0078799

mol of Zn left = 0.03059-0.0078799 = 0.02271

excess zin mass = mol*MW = 0.02271*65.38 = 1.484779 g of Zn left/excess

B)

0.0078799 mol of I2 react

c)

mol of Zn reacts = 0.0078799

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