`245g` pure `KClO_(3)` decomposes to give `48g` `O_2` .What is the % yield of reaction?

KClO_(3) on heating decomposes to give KCl and O_(2) . What is the volume of O_(2) at N.T.P liberated by 0.1 mole of KClO_(3) ?

KClO_(3) decomposes to KCl and O_(2) . If the volume of O_(2) obtained in this reaction is 1.12 lit at STP, weight of KCl formed in the reaction is

Gaseous ozone is bubbled through water-ice mixture at 0^@C . As the O_3(g) decomposes to form O_2 (g), the enthalpy of reaction is absorbed by the resulting ice. Given that the heat of fusion of ice is 6.0095 kJ "mol"^(-1) , calculate the mass of ice that melts for each gram of O_3 that decomposes. 2O_3(g) to 3O_2(g) , Delta H = -285.kJ

Fe_(2)O_(3) reacts with excess CO at a high temperature according to the equation below: Fe_(2)O_(3) + 3CO rightarrow 2Fe + 3CO_(2) If 6.5-0g of Fe_(2)O_(3) yields 3.85g of Fe, what is the percentage yield of the reaction ?

Write an expression for instantaneous rate of reaction: 2N_2O_5(g) to 4NO_2(g) + O_2(g). What is the order of reaction?

When KClO_(3) is heated, it decomposes into KCl+O_(2) , if some MnO_(2) is added, the reaction goes much faster because.