The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined. Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons. Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound. The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it. The amount of substance containing 12 g of pure carbon is called a mole. One mole of substance always contains 6 .022 × 10 23 atoms. Hence, ( 6 .022 × 10 23 atoms ) ( 12 u 1 atom ) = 12 g ⇒ 1 u = 1 6 .022 × 10 23 g To determine : The mass of nitrogen ( N ) in 5 .00 moles of NH 3 .
The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined. Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons. Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound. The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it. The amount of substance containing 12 g of pure carbon is called a mole. One mole of substance always contains 6 .022 × 10 23 atoms. Hence, ( 6 .022 × 10 23 atoms ) ( 12 u 1 atom ) = 12 g ⇒ 1 u = 1 6 .022 × 10 23 g To determine : The mass of nitrogen ( N ) in 5 .00 moles of NH 3 .
Solution Summary: The author explains that the number of moles of a compound is given and the mass of nitrogen in each compound given in exercise 51 is determined.
Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined.
Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.
Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.
The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.
The amount of substance containing
12g of pure carbon is called a mole. One mole of substance always contains
6.022×1023 atoms.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The mass of nitrogen
(N) in
5.00 moles of
NH3.
(b)
Interpretation Introduction
Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined.
Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.
Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.
The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.
The amount of substance containing
12g of pure carbon is called a mole. One mole of substance always contains
6.022×1023 atoms.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The mass of nitrogen
(N) in
5.00 moles of
N2H4.
(c)
Interpretation Introduction
Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined.
Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.
Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.
The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.
The amount of substance containing
12g of pure carbon is called a mole. One mole of substance always contains
6.022×1023 atoms.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The mass of nitrogen
(N) in
5.00 moles of
(NH4)2Cr2O7.
Below is the SN1 reaction of (S)-3-chlorocyclohexene and hydroxide (OH). Draw the missing curved arrows, lone pairs of electrons, and nonzero
formal charges. In the third box, draw the two enantiomeric products that will be produced.
5th attempt
Please draw all four bonds at chiral centers.
Draw the two enantiomeric products that will be produced. Draw in any hydrogen at chiral centers.
1000
4th attempt
Feedback
Please draw all four bonds at chiral centers.
8.
R5
HO:
See Periodic Table
See Hint
H
Cl
Br
Jid See Periodic Table See Hint
Show that a molecule with configuration π4 has a cylindrically symmetric electron distribution. Hint: Let the π orbitals be equal to xf and yf, where f is a function that depends only on the distance from the internuclear axis.
(a) Verify that the lattice energies of the alkali metal iodides are inversely proportional to the distances between the ions in MI (M = alkali metal) by plotting the lattice energies given below against the internuclear distances dMI. Is the correlation good? Would a better fit be obtained by plotting the lattice energies as a function of (1 — d*/d)/d, as theoretically suggested, with d* = 34.5 pm? You must use a standard graphing program to plot the graph. It generates an equation for the line and calculates a correlation coefficient. (b) From the graph obtained in (a), estimate the lattice energy of silver iodide. (c) Compare the results of (b) with the experimental value of 886 kJ/mol. If they do not agree, explain the deviation.