Answer:
V ≈ 646.50 L
General Formulas and Concepts:
<u>Chemistry - Gas Laws</u>
- Reading a Periodic Table
- Stoichiometry
- Combined Gas Law: PV = nRT
- R constant - 62.4 (L · torr)/(mol · K)
- Kelvin Conversion: K = °C + 273.15
Explanation:
<u>Step 1: Define</u>
RxN: N₂H₄ (g) + O₂ (g) → N₂ (g) + 2H₂O (l)
Given: 34.9 °C, 755.08 torr, 914.894 g H₂O
<u>Step 2: Identify Conversions</u>
Kelvin Conversion
Molar Mass of H - 1.01 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol
<u>Step 3: Convert</u>
Stoichiometry: 
= 25.3955 mol N₂
Temperature: 34.9 + 273.15 = 308.05 K
<u>Step 4: Find Volume</u>
- Substitute variables: (755.08 torr)V = (25.3955 mol)(62.4 (L · torr)/(mol · K))(308.05 K)
- Multiply: (755.08 torr)V = 488160 L · torr
- Isolate <em>V</em>: V = 646.502 L
<u>Step 5: Check</u>
<em>We are given 5 sig figs as our lowest. Follow sig fig rules and round.</em>
646.502 L ≈ 646.50 L
Answer:
4. Principal and Azimuthal (subsidiary) quantum number
5.Principal, Azimuthal (subsidiary), and magnetic quantum number
6. 10 electrons
7. 32 electrons
8. 36 electrons
Explanation:
4. Principal and Azimuthal (subsidiary) quantum number because in 4d, 4 represent principal quantum number and d- represents azimuthal quantum number (having l- value as 3)
5.Principal, Azimuthal (subsidiary), and magnetic quantum number are the first three because 2 stands for principal, s-for azimuthal (l=0) and magnetic quantum number for s- orbital= 0
6. 10 electrons, because for sublevel with l= 3, is a d-sub-level, and d- can take 10-electrons
7. 32 electrons, using the relationship 2×n^2 for the maximum number of electrons in a shell,
,n= 4 , hence 2×4^2= 32
8. 36 electrons, because n=4 and n= 3 can have the maximum configuration of [Ar]4s^2 3d^10 4p^6
This will sum up to 36- electrons, since Argon has 18 -electrons.
18+2+10+6=36 electrons
Answer: 0.08695652
Explanation:
You would do the answer you got subtracting from the expected answer over your expected answer
Answer:
The further an electron is from the nucleus. the greater its energy level.
Explanation:
When an electron is close to the nucleus, it is at as low an energy level as it can get.
We must put energy into an electron to pull it away from the attraction of a nucleus.
So, electrons that are further from the nucleus are at higher energy levels.
44. (a) N2O3 (b) SF4 (c) AlCl3 (d) Li2CO3
46. H Br
δ+ δ−
48. The metallic potassium atoms lose one electron and form +1 cations,
and the nonmetallic fluorine atoms gain one electron and form –1 anions.
K → K+
+ e–
19p/19e–
19p/18e–
F + e–
→ F–
9p/9e–
9p/10e–
The ionic bonds are the attractions between K+
cations and F–
anions.
50. See Figure 3.6.
52. (a) covalent…nonmetal-nonmetal (b) ionic…metal-nonmetal
54. (a) all nonmetallic atoms - molecular (b) metal-nonmetal - ionic
56. (a) 7 (b) 4
58. Each of the following answers is based on the assumption that nonmetallic
atoms tend to form covalent bonds in order to get an octet (8) of
electrons around each atom, like the very stable noble gases (other than
helium). Covalent bonds (represented by lines in Lewis structures) and lone
pairs each contribute two electrons to the octet.
(a) oxygen, O
If oxygen atoms form two covalent bonds, they will have an octet of electrons
around them. Water is an example:
H O H
(b) fluorine, F
If fluorine atoms form one covalent bond, they will have an octet of electrons
around them. Hydrogen fluoride, HF, is an example:
H F
(c) carbon, C
If carbon atoms form four covalent bonds, they will have an octet of electrons
around them. Methane, CH4, is an example:
H H
H
H
C
(d) phosphorus, P
If phosphorus atoms form three covalent bonds, they will have an octet
