A student attempted to identify an unknown compound by the method used in this e

Question

A student attempted to identify an unknown compound by the method used in this experiment. She found that when she heated a sample weighing 0.5032 g, the mass dropped to 0,2663 g. When the product was converted to a chloride, the mass went back up to 0.3747 g. Is the sample a carbonate? Please provide your reasoning below. Compound looses its mass when is heated, it means that we have of the compound because in dehydnatation when the compound water, the mass is decreased. What are the compounds that might be in the unknown? Write the balanced chemical equation for the overall reaction that occurs when each of these two original compounds is a hydrogen carbonate, use the sum of reactions 1 and 2. If the sample is a carbonate, use reaction 2. Write the equation for a sodium salt and then for a potassium salt. Reaction 1: 2 NaHCO3 rightarrow Na2 CO3 + CO_2 + H_2O 2KHCO3 rightarrow K2CO3 + CO_2 + H_2O Reaction 2: Na2 CO3(s) + 2H(ag) + 2cl^-(ag) rightarrow 2 NaCl(s) + H_2O(g) + CO_2(g) K2CO3(s) + 2H(ag) + 2Cl^-(ag) rightarrow 2Kcl (s) + H_2O(g) + CO_2 How many moles of the chloride salt would be produced from one mole of the original compound? How many grams of the chloride salt would be produced from one molar mass of the original compound? Molar masses: NaHCO3_g/mol Na2CO3_g/mol NaCL_g/mol If a sodium salt,_g original compound rightarrow_g chloride If a potassium salt,_g original compound rightarrow_g chloride

Explanation / Answer

Molar masses

If 58.44g of NaCl original compound ---> 35.5 g Chloride

if 74.5513g of KCl origial compound --> 35.5 g Chloride

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