The chemical equation is:
Sn + 4 HNO3 = SnO2 + 4 NO2 + 2 H2O
SnO2, if you meant (tin(IV) oxide) or tin dioxide that is
The ionic compound SnO2 is called tin(IV) oxide, also known as stannic oxide or dioxide.
To find the number of formula units in 22.4 g of SnO2, you first need to calculate the molar mass of SnO2. Sn has a molar mass of 118.71 g/mol and O has a molar mass of 16.00 g/mol. So, the molar mass of SnO2 is 134.71 g/mol. Next, divide the given mass by the molar mass to get the number of moles, then use Avogadro's number (6.022 x 10^23) to convert moles to formula units.
First of all, the correct formula is SnO2, and the Stock name is tin(IV) oxide.
There are approximately 3.02 x 10^24 oxygen atoms in 3.15 mol of SnO2. This is calculated by multiplying Avogadro's number (6.022 x 10^23) by the number of moles of oxygen atoms in SnO2 (2 moles of oxygen per 1 mole of SnO2).
Balanced equation: 2 H2 + O2 --> 2 H2O
In SnO2, the individual ions are Sn^4+ and O^2-. The tin ion has a charge of +4, while the oxygen ion has a charge of -2 to balance the overall charge of the compound.
To find the grams of Sn formed, we first need to calculate the number of moles of SnO2 in 12.5 grams. Then, we use the stoichiometry of the reaction to relate the number of moles of SnO2 to the number of moles of Sn. Finally, we convert the moles of Sn to grams using the molar mass of Sn.
SnO2, if you meant (tin(IV) oxide) or tin dioxide that is
The ionic compound SnO2 is called tin(IV) oxide, also known as stannic oxide or dioxide.
SnO2
SnBr4 + 2MgO -> SnO2 + 2MgBr2
First of all, the correct formula is SnO2, and the Stock name is tin(IV) oxide.
To find the number of formula units in 22.4 g of SnO2, you first need to calculate the molar mass of SnO2. Sn has a molar mass of 118.71 g/mol and O has a molar mass of 16.00 g/mol. So, the molar mass of SnO2 is 134.71 g/mol. Next, divide the given mass by the molar mass to get the number of moles, then use Avogadro's number (6.022 x 10^23) to convert moles to formula units.
The principal mineral of tin is cassiterite (SnO2).
Tin(II) oxide or tin dioxide
Hydrochloric acid is commonly used to dissolve tin oxide. Hydrochloric acid reacts with the tin oxide to form soluble tin chloride and water. Be sure to handle acids safely and use appropriate protective equipment.