Write a balanced chemical reaction showing how the 4.99 g Sn dissolves in HNO3.

To write a balanced chemical reaction showing how tin (Sn) dissolves in nitric acid (HNO3), we need to take into account the reactants and products involved.

The chemical formula for tin is Sn, and the chemical formula for nitric acid is HNO3.

The balanced chemical equation for the reaction can be written as follows:

Sn + 4 HNO3 → Sn(NO3)2 + 2 H2O + NO

In this equation, one molecule of tin reacts with four molecules of nitric acid to form one molecule of tin(II) nitrate (Sn(NO3)2), two molecules of water (H2O), and one molecule of nitrogen monoxide (NO).

To determine the coefficients of the balanced equation, we need to consider the stoichiometry of the reaction. Given that the mass of tin is 4.99 g, we can use the molar mass of tin (118.71 g/mol) to calculate the moles of tin present:

moles of Sn = mass of Sn / molar mass of Sn
moles of Sn = 4.99 g / 118.71 g/mol
moles of Sn = 0.042 moles

From the balanced equation, we can see that the stoichiometric ratio between tin and nitric acid is 1:4. Therefore, the moles of nitric acid required can be calculated as follows:

moles of HNO3 = moles of Sn × (4 moles of HNO3 / 1 mole of Sn)
moles of HNO3 = 0.042 moles × (4 moles of HNO3 / 1 mole of Sn)
moles of HNO3 = 0.168 moles

Now that we have the moles of tin and nitric acid, we can write the balanced chemical equation showing the reaction in terms of moles:

0.042 moles Sn + 0.168 moles HNO3 → 0.042 moles Sn(NO3)2 + 0.084 moles H2O + 0.042 moles NO

Finally, to convert the balanced chemical equation from moles to grams, we can multiply the number of moles by the molar mass of each substance involved.

I hope this helps! Let me know if you have any other questions.

To write a balanced chemical reaction showing how tin (Sn) dissolves in nitric acid (HNO3), we need to follow a few steps:

Step 1: Determine the balanced formula equation for the reaction.
The reaction involves tin (Sn) reacting with nitric acid (HNO3). Nitric acid is a strong acid that can donate a proton (H+) in solution. However, tin is a metal, and metals do not typically react with acids to produce hydrogen gas (H2) like non-metals do.

Instead, when tin reacts with nitric acid, it undergoes an oxidation-reduction reaction, also known as a redox reaction. In this reaction, tin gets oxidized, while the nitric acid gets reduced.

The balanced equation for this redox reaction can be represented as follows:
Sn + 4HNO3 -> Sn(NO3)2 + 2NO2 + 2H2O

Step 2: Determine the molar mass of Sn.
The molar mass of tin (Sn) is 118.71 g/mol. This value can be found using the periodic table, where the atomic mass of tin is given.

Step 3: Calculate the number of moles of Sn.
To determine the number of moles, we can use the formula:
moles = mass / molar mass

Given that the mass of Sn is 4.99 g, we can substitute it into the formula:
moles of Sn = 4.99 g / 118.71 g/mol

Step 4: Use the balanced equation to find the coefficients that correspond to the moles of Sn.
From the balanced equation, we can see that the stoichiometric ratio between tin (Sn) and Sn(NO3)2 is 1:1. This means that 1 mole of Sn will produce 1 mole of Sn(NO3)2.

Step 5: Calculate the number of moles of Sn(NO3)2.
Since the stoichiometric ratio between Sn and Sn(NO3)2 is 1:1, the moles of Sn(NO3)2 will be the same as the moles of Sn calculated in Step 3.

moles of Sn(NO3)2 = moles of Sn (from step 3)

Step 6: Calculate the mass of Sn(NO3)2.
To determine the mass of Sn(NO3)2, we can use the formula:
mass = moles x molar mass

Given that the molar mass of Sn(NO3)2 is 238.69 g/mol, we can substitute the values into the formula:
mass of Sn(NO3)2 = moles of Sn(NO3)2 x molar mass of Sn(NO3)2

Step 7: Substitute the values into the balanced chemical equation.
Considering the equation Sn + 4HNO3 -> Sn(NO3)2 + 2NO2 + 2H2O, we have calculated the moles and mass of Sn as well as the moles and mass of Sn(NO3)2. We can now substitute these values into the equation.

Substituting the mass of Sn (4.99 g Sn) and the mass of Sn(NO3)2 (from step 6) into the equation, we get:

4.99 g Sn + 4HNO3 -> mass of Sn(NO3)2 + 2NO2 + 2H2O

Please note that the mass of Sn(NO3)2 will depend on the calculated moles and molar mass.

Sn + HNO3 ==> Sn^+2 + NO + H2O

You balance.