Answer:
1.852 g of CO2 were produced in the chemical reaction
Explanation:
The problem is pretty simple. We can write down the chemical reaction that is involved to help us understand better what is going on in the process:
CaCO3 (aq) + HAc (aq) → CaAc (aq) + CO2 (g) + H2O (l)
Let's think this through: we have a tablet that has an active compound (CaCO3) and an inert substance that weighs 0.833 g. When we add 58.072 g of an acid solution (represented in the equation as HAc because we are not told specifically which acid is being added), CO2 is formed and released from solution as gas leaving us with an aqueous solution that weighs 57.053 g.
Having said that, we know that the only mass lost during the reaction is due to the formation of CO2 gas. Therefore, we sum the reactants (the tablet + the acid solution) and subtract the mass of the remnant solution. This value will indicate us the amount of CO2 formed:
0.833 g of the Tablet + 58.072 g from the Acid solution = 58.905 g
58.905 g of reactants - 57.053 g of remnant solution = 1.852 g of produced CO2.
The inner core has the greatest pressure.
and 
are polyatomic anions composed of two or more atoms.
<h3>What is a polyatomic anion?</h3>
A polyatomic ion is an ion composed of two or more atoms. Examples: The hydroxide cation (
) and the phosphate cation (
) are both polyatomic ions.
and are the polyatomic anions because both contain more than 1 atom.
Hence,
and are polyatomic anions composed of two or more atoms.
Learn more about the polyatomic anion here:
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Answer:
∴ No. of atoms in 0.01 moles of NaOH = 6.02×10
23
×0.01=6.02×10
21
The balanced equation is:
BaCl2 (aq) + Na2SO4 (aq) ----> BaSO4(s)+ 2 NaCl(aq)
This is a double replacement reaction.
The reactants are:
a) BaCl2: barium chloride, a ionic compound, therefore soluble in water,
b) Na2SO4: sodium sulfate, another ionic compound, therefore also soluble in water.
The products are:
c) BaSO4: barium sulfate, a solid not soluble in water which precipitates.
d) NaCl: sodium chloride, an ionic compound, therefore soluble in water.
