silvajimena74

28.02.2020 • 

Chemistry

1. When aqueous solutions of potassium carbonate and calcium nitrate are combined, solid calcium carbonateand a solution of potassium nitrate are formed. The net ionic equation for this reaction is:

2. When aqueous solutions of potassium nitrite and nitric acid are mixed, an aqueous solution of potassiumnitrate and nitrous acid results. Write the net ionic equation for the reaction.

3.
When solid Mg metal is put into an aqueous solution of Pb(NO3)2, solid Pb metal and a solution of Mg(NO3)2result. Write the net ionic equation for the reaction.

4. Consider the reaction when aqueous solutions of chromium(III) bromide and silver(I) acetate are combined. The net ionic equation for this reaction is:

5. Consider the reaction when aqueous solutions of barium nitrate and potassium bromide are combined. The net ionic equation for this reaction is:

6. Consider the reaction when aqueous solutions of barium acetate and iron(II) bromide are combined. The net ionic equation for this reaction is:

7. Consider the reaction when aqueous solutions of iron(II) nitrate and aluminum sulfate are combined. The net ionic equation for this reaction is:

8. Consider the reaction when aqueous solutions of cobalt(II) acetate and chromium(III) sulfate are combined. The net ionic equation for this reaction is:

Ответ:

bestsisever0

22.04.2020

Chemistry

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k n kk u

Explanation:

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Ответ:

adriana145

23.05.2022

Chemistry

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11.58 g

Explanation:

CaO + H₂O→ Ca(OH)₂

First we convert the given masses of both reactants into moles, using their respective molar masses:

6.89 g CaO ÷ 56 g/mol = 0.123 mol CaO13.79 g H₂O ÷ 18 g/mol = 0.766 mol H₂O

As 1 H₂O mol reacts completely with 1 CaO mol, and there are more H₂O moles than CaO moles, water is the non limiting reactant.

We calculate the mass of the reacting moles of water (the same number of CaO moles, 0.123):

0.123 mol H₂O * 18 g/mol = 2.21 g

Finally we calculate how many grams of water remained after the reaction:

13.79 g - 2.21 g = 11.58 g

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