Determine the mass of copper(ii)trioxonitrate(v) that will be formed when 15grams of copper is added to excess dilute trioxonitrate(v).{cu=63.5,N=14,O=16} solution cu(No3)2=Cu N2 O6 =63.5+14x2+16x6 =63.5+28+96 =187.5 Number of mole=mass/molar mass =15/187.5 =0.08mol.
Solut its
To determine the mass of copper(II) trioxonitrate(V) (Cu(NO3)2) that will be formed, we need to use stoichiometry.
The balanced chemical equation for the reaction between copper (Cu) and trioxonitrate(V) (NO3) is:
Cu + 2NO3 -> Cu(NO3)2
From the balanced equation, we can see that 1 mole of copper reacts with 2 moles of trioxonitrate(V) to form 1 mole of copper(II) trioxonitrate(V).
Given that the number of moles of copper (Cu) is 0.08 mol (calculated from 15g Cu and molar mass of Cu), we can use the stoichiometry of the reaction to determine the number of moles of copper(II) trioxonitrate(V) formed.
Using the stoichiometry, we have:
0.08 mol Cu x (1 mol Cu(NO3)2 / 1 mol Cu) = 0.08 mol Cu(NO3)2
Finally, to calculate the mass of copper(II) trioxonitrate(V):
Mass = Number of moles x molar mass
= 0.08 mol x (63.5 + (14 x 2) + (16 x 6))
= 0.08 mol x 187.5 g/mol
= 15 g
Therefore, the mass of copper(II) trioxonitrate(V) formed when 15 grams of copper is added to an excess of dilute trioxonitrate(V) is also 15 grams.
To determine the mass of copper(II) trioxonitrate(V) that will be formed when 15 grams of copper is added to an excess of dilute trioxonitrate(V) solution, we first need to calculate the molar mass of copper(II) trioxonitrate(V).
The formula of copper(II) trioxonitrate(V) is Cu(NO3)2. From the formula, we know that copper (Cu) has a molar mass of 63.5 g/mol, nitrogen (N) has a molar mass of 14 g/mol, and oxygen (O) has a molar mass of 16 g/mol.
To calculate the molar mass of copper(II) trioxonitrate(V), we multiply the atomic masses of each element by the number of atoms present in the formula. In this case, there is 1 copper atom (63.5 g/mol), 2 nitrogen atoms (14 g/mol x 2), and 6 oxygen atoms (16 g/mol x 6).
Molar mass of Cu(NO3)2:
= (63.5 g/mol) + (14 g/mol x 2) + (16 g/mol x 6)
= 63.5 g/mol + 28 g/mol + 96 g/mol
= 187.5 g/mol
Next, we need to calculate the number of moles of copper that reacted. We are given that the mass of copper is 15 grams.
Number of moles = mass / molar mass
Number of moles = 15 g / 187.5 g/mol
Number of moles = 0.08 mol
Finally, we can calculate the mass of copper(II) trioxonitrate(V) formed using the molar ratio between copper and copper(II) trioxonitrate(V).
From the balanced chemical equation, we can see that the ratio is 1:1. This means that for every 1 mol of copper, we get 1 mol of copper(II) trioxonitrate(V).
Mass of copper(II) trioxonitrate(V) = number of moles x molar mass
Mass of copper(II) trioxonitrate(V) = 0.08 mol x 187.5 g/mol
Mass of copper(II) trioxonitrate(V) = 15 g
Therefore, the mass of copper(II) trioxonitrate(V) formed is 15 grams.