KClO_(3)longrightarrow KCl+O_(2)

Balance the following chemical equations. d) KClO_(3)rarr KCl +O_(2)

Which of the followings are disproportionation reactions? (A) \(2O_{3} \rightarrow 3O_{2}\) (B) \(KClO_{3} \rightarrow 3KClO_{4}+KCl\) (C)\(2H_{2}O_{2}\rightarrow2H_{2}O+O_{2}\) (D) \(2KO_{2}+2H_{2}O\rightarrow4KOH+3O_{2}\)

The decomposition of KClO_(3) to KCl and O_(2) on heating is an example of :

The decomposition of KClO_(3) to KCl and O_(2) on heating is an example of :

Balance the following equation : KClO_(3) to KCl + O_(2)

KClO_(3) to KCl + O_(2) (unbalanced), If in above reaction 5 moles of KClO_(3) was heated, then find moles of O_(2) produced on completion of reaction.

Equal masses of KClO_(3) undergoes different reaction in two different container: (i) 2KClO_(3) to 2KCl + 3O_(2) (ii) 4KClO_(3)to KCl + 3KClO_(4) Mass ratio of the KCl produced in respective reaction is x : 1. Value of 'x' will be

2 g sample of KClO_(3) was heated under such conditions that a part of it decomposed according to the equation : 2KClO_(3) rarr 2KCl + 3O_(2) and the remaining underwent change according to the equation : 4KClO_(3)rarr 3KClO_(4)+KCl If the amount of O_(2) evolved was 146.8 ml at S.T.P., calculate the % by weight of KClO_(4) in the reside.