Respuesta :
The balanced chemical reaction is given as follows:
2 KClO3(s) → 2 KCl(s) + 3 O2(g)
The starting amount of the reactant are given above. These values would be used for the calculations. We do as follows:
2.72 g KClO3 (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 1.06 g O2
0.361 g KClO3 (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 0.14 g O2
83.6 kg KClO3 (1000g / 1kg) (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 3275.76 g O2
22.5 mg KClO3 (1 g / 1000 mg) (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 0.009 g O2
2 KClO3(s) → 2 KCl(s) + 3 O2(g)
The starting amount of the reactant are given above. These values would be used for the calculations. We do as follows:
2.72 g KClO3 (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 1.06 g O2
0.361 g KClO3 (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 0.14 g O2
83.6 kg KClO3 (1000g / 1kg) (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 3275.76 g O2
22.5 mg KClO3 (1 g / 1000 mg) (1 mol / 122.50g )( 3 mol O2 / 2 mol KClO3 ) ( 32 g O2 / 1 mol O2 ) = 0.009 g O2
Answer :
The mass of oxygen form from 2.72 g [tex]KClO_3[/tex] is 1.06 grams.
The mass of oxygen form from 0.361 g [tex]KClO_3[/tex] is 0.141 grams.
The mass of oxygen form from 83.6 kg [tex]KClO_3[/tex] is 32.7 kilograms.
The mass of oxygen form from 22.5 mg [tex]KClO_3[/tex] is 8.81 milligrams.
Explanation :
The given chemical reaction is:
[tex]2KClO_3(s)\rightarrow 2KCl(s)+3O_2(g)[/tex]
Molar mass of [tex]KClO_3[/tex] = 122.55 g/mol
Molar mass of [tex]O_2[/tex] = 32 g/mol
For 2.72 g [tex]KClO_3[/tex] :
From the balanced chemical reaction we conclude that,
As, [tex]2\times 122.55[/tex] grams of [tex]KClO_3[/tex] decomposes to give [tex]3\times 32[/tex] grams of [tex]O_2[/tex]
So, [tex]2.72[/tex] grams of [tex]KClO_3[/tex] decomposes to give [tex]\frac{3\times 32}{2\times 122.55}\times 2.72=1.06[/tex] grams of [tex]O_2[/tex]
Thus, the mass of oxygen form from 2.72 g [tex]KClO_3[/tex] is 1.06 grams.
For 0.361 g [tex]KClO_3[/tex] :
From the balanced chemical reaction we conclude that,
As, [tex]2\times 122.55[/tex] grams of [tex]KClO_3[/tex] decomposes to give [tex]3\times 32[/tex] grams of [tex]O_2[/tex]
So, [tex]0.361[/tex] grams of [tex]KClO_3[/tex] decomposes to give [tex]\frac{3\times 32}{2\times 122.55}\times 0.361=0.141[/tex] grams of [tex]O_2[/tex]
Thus, the mass of oxygen form from 0.361 g [tex]KClO_3[/tex] is 0.141 grams.
For 83.6 kg [tex]KClO_3[/tex] :
From the balanced chemical reaction we conclude that,
As, [tex]2\times 122.55[/tex] grams of [tex]KClO_3[/tex] decomposes to give [tex]3\times 32[/tex] grams of [tex]O_2[/tex]
So, [tex]83.6kg[/tex] of [tex]KClO_3[/tex] decomposes to give [tex]\frac{3\times 32}{2\times 122.55}\times 83.6=32.7kg[/tex] of [tex]O_2[/tex]
Thus, the mass of oxygen form from 83.6 kg [tex]KClO_3[/tex] is 32.7 kilograms.
For 22.5 mg [tex]KClO_3[/tex] :
From the balanced chemical reaction we conclude that,
As, [tex]2\times 122.55[/tex] grams of [tex]KClO_3[/tex] decomposes to give [tex]3\times 32[/tex] grams of [tex]O_2[/tex]
So, [tex]22.5mg[/tex] of [tex]KClO_3[/tex] decomposes to give [tex]\frac{3\times 32}{2\times 122.55}\times 22.5=8.81mg[/tex] of [tex]O_2[/tex]
Thus, the mass of oxygen form from 22.5 mg [tex]KClO_3[/tex] is 8.81 milligrams.
