The mass of hydrogen is 16.0 oz. To convert 16.0 oz of hydrogen into pounds, we utilize the conversion factor 1 lb = 16 oz. Next, we convert pounds to grams using the factors 1 kg = 2.2 lb and 1 kg = 1000 g. The heat of combustion for hydrogen is 142 J/g, and we will calculate the heat produced by combusting 16.0 oz.
Answer:
Can you rank the following chemical substances in order of their absolute entropies (So) from lowest (1) to highest (5) at a temperature of 298 K?
a. Al (s)
b. H2O (l)
c. HCN (g)
d. CH3COOH (l)
e. C2H6 (g)
Explanation:
Entropy quantifies the level of disorder within a system.
In solids, the entropy is significantly lower compared to liquids and gases.
The typical order of entropy is:
solids < liquids < gases
In the substances listed, liquid water notably exhibits strong intermolecular hydrogen bonding.
This results in water having comparatively lower entropy.
Next in line is acetic acid.
Among the gaseous components, ethane has higher entropy than HCN due to its weaker intermolecular interactions.
HCN involves some hydrogen bonding.
Thus, the order of entropy is:
Al(s) < CH3COOH (l) < H2O(l) < HCN(g) < C2H6(g)
Answer:
The correct choice is: option A.
Justification:
To address this inquiry, we need to evaluate the total number of electrons each orbital can accommodate.
Orbital Number of electrons
s 2
p 6
d 10
f 14
Provided options:
A. 1s² 2s² 2p⁶ 3s² This configuration is valid as it aligns with the permitted number of electrons in each orbital and follows the correct sequence.
B. 1s² 2s² 2p⁶ 3s² 3d⁴ This configuration is not accurate because
3d⁴ should follow 3p.
C. 1s² 2s² 2d¹⁰ 2p³ This is incorrect since 2d¹⁰ is not a valid orbital.
D. 1s² 2s^s 2p³ 2d¹⁰ This option contains two errors; s as an exponent does not exist, and 2d¹⁰ is also an invalid description.
Answer:
Explanation:
The percent composition indicates the mass percentage of a specific element within the compound.
The chemical formula for chromium(III) nitrate is 
.
The molar mass for chromium(III) nitrate is calculated at 238.011 g/mol.
Each mole of chromium(III) nitrate includes 9 moles of oxygen.
The molar mass of oxygen is 16 g/mol.
Hence, Mass = Molar mass * Moles = 16 * 9 g = 144 g.
