Question #171592

2g of a mixture of KCLO3 and KCL yielded 336cm^3 of O2 measured dry at 747mmHg on heating. Calculate the volume of dry O2 measured at stp and the percentage composition of KCLO3.


1
Expert's answer
2021-03-17T06:44:59-0400

2KClO3 → 2KCl + 3O2

We will use the temperature value of 127 ºC.

T = 127 + 273 = 400 K

P = 747 mmHg = 0.982 atm

V = 336 mL = 0.336 L

Ideal Gas Law

PV = nRT

R = 0.08206 L×atm/mol×K

n=PVRTn(O2)=0.982×0.3360.08206×400=0.01  moln = \frac{PV}{RT} \\ n(O_2) = \frac{0.982 \times 0.336}{0.08206 \times 400} \\ = 0.01 \;mol

At STP one mole of any gas occupies volume of 22.4 L.

At STP V(O2)=0.01×22.4=0.224  L=224  mLV(O_2) = 0.01 \times 22.4 = 0.224 \;L = 224 \;mL

According to the reaction:

n(KClO3) =23n(O2)=230.01=0.0066  mol= \frac{2}{3}n(O_2) = \frac{2}{3}0.01= 0.0066 \;mol

M(KClO3) = 122.55 g/mol

m(KClO3)=n×M=0.0066×122.55=0.817  gm(KClO_3) = n \times M = 0.0066 \times 122.55 = 0.817 \;g

Proportion:

2 g – 100 %

0.817 g – x

x=0.817×1002=40.8  %x = \frac{0.817 \times 100}{2} = 40.8 \; \%



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