What is the net ionic of 2HCl + K2CO3 -> 2KCl + CO2 +H2O? or do I just put no reaction?
Answer:
Explanation:
Step to write ionic equation equation:
Step 1: Write the balanced chemical equation
K2CO3(aq) +2 HCl(aq) -> 2 KCl(aq) + CO2(g) + H2O(l)
Step 2: Write the ionic equation.
2K+(aq) + CO3 -2(aq) +2H+(aq) + 2Cl-(aq) --------> 2K+(aq) + 2Cl -(aq) + CO2(g) + H2O(l)
[ Here, aqueous compounds will breaks and solid,liquid and gaseous compound will remain unchanged. So K2CO3 (aq) and 2KCl(aq) and 2HCl(aq) wil breaks into ions ]
Step 3: Write the net ionic equation
[ net ionic equation is written by crossing out the spectator ions from the complete ionic equation ]
You can recognize spectator ions by looking for ions that are present on both sides of the equation. They will always have the same exact formula, charge, and physical state.
2K+(aq) + CO3 -2(aq) +2H+(aq) + 2Cl-(aq) --------> 2K+(aq) + 2Cl -(aq) + CO2(g) + H2O(l)
Final net ionic equation
CO3 -2(aq) +2H+(aq) --------> CO2(g) + H2O(l)
4. What is the net ionic equation for the following reaction? (2 Pts.) K2CO3 (aq) + H2SO4 (aq) → K2SO4 (aq) + CO2 (g) + H2O (2) 5. An unknown gas has a density of 0.355 g/L at 17 °C and 189 mm Hg. (i) Calculate the molar mass of the gas? (ii) What is the identity of the gas? (2 pts.)
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Consider the reaction of CO2 with KOH to form K2CO3 and H2O. If 3.80 g KOH is reacted with excess CO2 and 4.27 g of K2CO3 is ultimately isolated, what is the percent yield for the reaction?
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The reaction is: K2CO3 + 2 NH4NO3 → 2 KNO3 + CO2 + H2O + 2 NH3. What is the mass of KNO3 that is produced from 1kg of potassium carbonate and 2kg of ammonium nitrate.?
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