Magnesium nitrate and barium nitrate decompose similarly on heating and the reaction can be represented as follow: M(NO3)2 (s) --› MO (s) + 2NO2 (g) + ½O2 (g), where M = Mg or Ba (a) When Group 1 nitrates (with the exception of lithium nitrate) are strongly heated, the corresponding nitrite was formed along with a colorless gas which relights a glowing splint. (i) Write a balanced equation for the thermal decomposition of potassium nitrate. (ii) Unlike other Group 1 nitrates, lithium nitrate decomposes on heating in the same way as Group 2 nitrates. Suggest a reason for the difference in behaviour, and give an equation for its decomposition.
Magnesium nitrate and barium nitrate decompose similarly on heating and the reaction can be represented as follow:
M(NO3)2 (s) --› MO (s) + 2NO2 (g) + ½O2 (g), where M = Mg or Ba
(a) When Group 1 nitrates (with the exception of lithium nitrate) are strongly heated, the corresponding nitrite was formed along with a colorless gas which relights a glowing splint.
(i) Write a balanced equation for the thermal decomposition of potassium nitrate.
(ii) Unlike other Group 1 nitrates, lithium nitrate decomposes on heating in the same way as Group 2 nitrates. Suggest a reason for the difference in behaviour, and give an equation for its decomposition.
(b) Zinc carbonate and magnesium carbonate decompose when heated to give similar products.
(i) Suggest an equation for the thermal decomposition of magnesium carbonate.
(ii) The radius of Zn2+ cation is 0.074 nm. Use the Data Booklet to deduce whether zinc carbonate will decompose at a higher or lower temperature than magnesium carbonate. Explain your answer.
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