Decomposition of Sodium Chlorate Lab
Decomposition of Sodium Chlorate
Mass, Moles, and the Chemical Equation
Introduction:
Sodium chlorate is used as a source of oxygen in emergency oxygen generators. So-called oxygen canisters or oxygen candles are found on airplanes, submarines, even the space station–anywhere where oxygen might be in short supply in case of an emergency. Sodium chlorate decomposes upon heating or in the presence of metals to give oxygen gas. What the chemical equation for the decomposition of sodium chlorate?
The purpose of this inquiry-based experiment is to design a small-scale procedure to determine the chemical equation for the thermal decomposition of sodium chlorate.
Background:
Sodium chlorate, NaClO3, is a colorless, odorless, white solid that melts at 248 °C. When heated above 300 °C, it begins to lose oxygen. The ultimate products of the thermal decomposition of sodium chlorate are oxygen gas and a white solid. Based on the molecular formula of sodium chlorate, three possible reactions will account for the loss of oxygen gas upon heating (Equations 1-3). Note that equations 1-3 are not balanced.
Equation 1 2NaClO3(s) → 2NaClO2(s) + O2(g)
Equation 2 NaClO3(s) → NaClO(s) + O2(g)
Equation 3 2NaClO3(s) → 2NaCl(s) + 3O2(g)
What is the actual chemical equation for the thermal decomposition of sodium chlorate? All of the possible sodium-containing products n Equations 1-2 are real compounds: sodium chlorite, NaClO2; sodium hypochlorite, NaClO; and sodium chloride, NaCl. All are white solids at room temperature. It is possible to determine the chemical equation for the decomposition of sodium chlorate by applying the principles of stoichiometry to the masses of the reactants and products.
Safety Precautions:
Sodium chlorate is a strong oxidizing agent and a dangerous fire risk; it is slightly toxic by ingestion. Contact with metal powders or combustible organic compounds may cause fires. Keep away from contact with organic
Mass, Moles, and the Chemical Equation
Introduction:
Sodium chlorate is used as a source of oxygen in emergency oxygen generators. So-called oxygen canisters or oxygen candles are found on airplanes, submarines, even the space station–anywhere where oxygen might be in short supply in case of an emergency. Sodium chlorate decomposes upon heating or in the presence of metals to give oxygen gas. What the chemical equation for the decomposition of sodium chlorate?
The purpose of this inquiry-based experiment is to design a small-scale procedure to determine the chemical equation for the thermal decomposition of sodium chlorate.
Background:
Sodium chlorate, NaClO3, is a colorless, odorless, white solid that melts at 248 °C. When heated above 300 °C, it begins to lose oxygen. The ultimate products of the thermal decomposition of sodium chlorate are oxygen gas and a white solid. Based on the molecular formula of sodium chlorate, three possible reactions will account for the loss of oxygen gas upon heating (Equations 1-3). Note that equations 1-3 are not balanced.
Equation 1 2NaClO3(s) → 2NaClO2(s) + O2(g)
Equation 2 NaClO3(s) → NaClO(s) + O2(g)
Equation 3 2NaClO3(s) → 2NaCl(s) + 3O2(g)
What is the actual chemical equation for the thermal decomposition of sodium chlorate? All of the possible sodium-containing products n Equations 1-2 are real compounds: sodium chlorite, NaClO2; sodium hypochlorite, NaClO; and sodium chloride, NaCl. All are white solids at room temperature. It is possible to determine the chemical equation for the decomposition of sodium chlorate by applying the principles of stoichiometry to the masses of the reactants and products.
Safety Precautions:
Sodium chlorate is a strong oxidizing agent and a dangerous fire risk; it is slightly toxic by ingestion. Contact with metal powders or combustible organic compounds may cause fires. Keep away from contact with organic