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 letter D because the more the N on the left have more on the right.
There are six atoms in the carbon
Answer:
Molecules in liquids are held to other molecules by intermolecular interactions, which are weaker than the intramolecular interactions that hold the atoms together within molecules and polyatomic ions.
To calculate number of moles, all you do is divide the given mass by the molecular molar mass:
<span>i.e. 125g / 18g = 6.94444g </span>
<span>Therefore, your answer is (a) 6.94 g</span>
