calculate the mass of zinc that will produce 35.8g of zinc trioxonitrate
The molecular formula of zinc trioxonitrate is Zn(NO3)2.
To calculate the mass of zinc required to produce 35.8g of zinc trioxonitrate, we need to determine the molar mass of the compound.
The molar mass of zinc (Zn) is 65.38 g/mol.
The molar mass of nitrate (NO3) is calculated as follows:
Molar mass of nitrogen (N) = 14.01 g/mol
Molar mass of oxygen (O) = 16.00 g/mol
Therefore, the molar mass of nitrate (NO3) = (14.01 g/mol) + (3 * 16.00 g/mol) = 62.01 g/mol.
The molar mass of zinc trioxonitrate (Zn(NO3)2) is therefore calculated as:
Molar mass = (Molar mass of zinc) + (2 * Molar mass of nitrate)
Molar mass = 65.38 g/mol + (2 * 62.01 g/mol) = 189.40 g/mol.
Now, we can calculate the mass of zinc required using the following formula:
Mass of zinc = (Mass of zinc trioxonitrate) * (Molar mass of zinc) / (Molar mass of zinc trioxonitrate)
Mass of zinc = 35.8g * 65.38 g/mol / 189.40 g/mol
Mass of zinc = 12.36 g
Therefore, approximately 12.36g of zinc will produce 35.8g of zinc trioxonitrate.
To calculate the mass of zinc required to produce 35.8g of zinc trioxonitrate, we need to use the balanced chemical equation for the reaction.
The balanced equation for the formation of zinc trioxonitrate (Zn(NO3)2) from zinc (Zn) is:
3Zn + 2HNO3 → Zn(NO3)2 + H2
From the equation, we can see that the molar ratio between zinc and zinc trioxonitrate is 3:1. This means that for every 3 moles of zinc, we obtain 1 mole of zinc trioxonitrate.
1 mole of zinc trioxonitrate has a molar mass of:
Zn(NO3)2 = (1 × atomic mass of Zn) + (2 × atomic mass of N) + (6 × atomic mass of O)
Zn(NO3)2 = (1 × 65.38 g/mol) + (2 × 14.01 g/mol) + (6 × 16.00 g/mol)
Zn(NO3)2 = 161.38 g/mol
Now, we can calculate the moles of zinc trioxonitrate produced:
moles of Zn(NO3)2 = mass of Zn(NO3)2 / molar mass of Zn(NO3)2
moles of Zn(NO3)2 = 35.8 g / 161.38 g/mol
To obtain the moles of zinc, we use the mole ratio of 3:1 between zinc and zinc trioxonitrate:
moles of Zn = (3/1) * moles of Zn(NO3)2
Finally, we can calculate the mass of zinc:
mass of Zn = moles of Zn × molar mass of Zn
Substituting the known values:
mass of Zn = ((3/1) * (35.8 g / 161.38 g/mol)) × 65.38 g/mol
Simplifying the equation:
mass of Zn = (3 * 35.8 g * 65.38 g) / (1 * 161.38 g)
Therefore, the mass of zinc required to produce 35.8g of zinc trioxonitrate is approximately equal to 52.9g.
To calculate the mass of zinc (Zn) required to produce a given mass of zinc trioxonitrate (Zn(NO3)2), we need to determine the chemical equation and the molar masses of both substances.
The chemical equation for the reaction between zinc and nitric acid to produce zinc trioxonitrate is:
Zn + 2HNO3 → Zn(NO3)2 + H2O
To calculate the mass of zinc trioxonitrate, we need to find the molar mass of Zn(NO3)2. The molar mass can be calculated by summing up the atomic masses of each element in the compound:
Molar mass of Zn(NO3)2 = (1 × Atomic mass of Zn) + (2 × Atomic mass of N) + (6 × Atomic mass of O)
Using the periodic table, the atomic masses are:
Atomic mass of Zn = 65.38 g/mol
Atomic mass of N = 14.01 g/mol
Atomic mass of O = 16.00 g/mol
Plugging in the values, we get:
Molar mass of Zn(NO3)2 = (1 × 65.38) + (2 × 14.01) + (6 × 16.00) = 189.38 g/mol
Now, we can use the molar mass of Zn(NO3)2 to calculate the amount of Zn required to produce a given mass of the compound.
Using the moles-to-mass ratio, we can convert the mass of Zn(NO3)2 to moles:
Moles of Zn(NO3)2 = Mass of Zn(NO3)2 / Molar mass of Zn(NO3)2
Moles of Zn(NO3)2 = 35.8 g / 189.38 g/mol
Next, we look at the balanced chemical equation to determine the mole ratio between Zn and Zn(NO3)2. From the equation, we can see that one mole of Zn reacts to form one mole of Zn(NO3)2.
Therefore, the moles of Zn required will be the same as the moles of Zn(NO3)2:
Moles of Zn = Moles of Zn(NO3)2
Finally, we can calculate the mass of zinc using the moles-to-mass ratio:
Mass of Zn = Moles of Zn × Molar mass of Zn
Mass of Zn = Moles of Zn × 65.38 g/mol
Substituting the moles value we previously calculated:
Mass of Zn = 35.8 g / 189.38 g/mol × 65.38 g/mol
Now you can solve this equation to find the mass of zinc required.