Answer:
37.8 L OF CARBON MONOXIDE IS REQUIRED TO PRODUCE 18.9 L OF NITROGEN.
Explanation:
Equation for the reaction:
2 CO + 2 NO ------> N2 + 2 CO2
2 moles of carbon monoxide reacts with 2 moles of NO to form 1 mole of nitrogen
At standard temperature and pressure, 1 mole of a gas contains 22.4 dm3 volume.
So therefore, we can say:
2 * 22.4 L of CO produces 22.4 L of N2
44.8 L of CO produces 22.4 L of N2
Since, 18.9 L of Nitrogen is produced, the volume of CO needed is:
44.8 L of CO = 22.4 L of N
x L = 18.9 L
x L = 18.9 * 44.8 / 22.4
x L = 18.9 * 2
x = 37.8 L
The volume of Carbon monoxide required to produce 18.9 L of N2 is 37.8 L
To finish calculating the frequency of an electromagnetic wave, you need the wavelength
First, we must find the total mass of CuBr₂:
Mass = 64 + 2 x 80
Mass = 224
Percentage mass of copper = mass of copper x 100 / total mass
Percentage mass of copper = (64 / 224) x 100
Percentage mass of copper = 28.45%
Answer:
6.75 moles of CuCl₂ were used
Explanation:
Given data:
Number of moles of AlCl₃ formed = 4.5 mol
Number of moles of CuCl₂ used = ?
Solution:
Chemical equation:
3CuCl₂ + 2Al → 2AlCl₃ + 3Cu
Now we will compare the moles of CuCl₂ and AlCl₃
AlCl₃ : CuCl₂
2 : 3
4.5 : 3/2×4.5 = 6.75
6.75 moles of CuCl₂ were used.
