How many grams of ca(no3)2 can be produced by reacting excess hno3 with 6.33 g of ca(oh)2?

Amount of Ca(NO3)2 produced = 14.02 g

Explanation:

The given reaction can be depicted as follows:

Ca(OH)2 + 2HNO3 → Ca(NO3)2 + 2H2O

Since it is given that HNO3 is in excess, the limiting reactant is Ca(OH)2

Now, Mass of Ca(OH)2 = 6.33 g

Molar mass of Ca(OH)2 = 74 g/mol

Based on the reaction stoichiometry:

1 mole of Ca(OH)2 forms 1 mole of Ca(NO3)2

Therefore, moles of Ca(NO3)2 produced from the moles of Ca(OH)2 reacted = 0.0855 moles

Molar mass of Ca(NO3)2 = 164 g/mol

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

c is the answer because when something is left after something evaporates that shows the chemical change.