Answer: The number of sulfur dioxide molecules present is 1.27·10²³.
Calculating: m(SO₂) equals 13.5 g.
Using the formula n(SO₂) = m(SO₂) ÷ M(SO₂).
This gives n(SO₂) = 13.5 g ÷ 64 g/mol.
Resulting in n(SO₂) = 0.21 mol.
Subsequently, N(SO₂) = n(SO₂) ·Na.
Therefore, N(SO₂) = 0.21 mol · 6.022·10²³ 1/mol.
Ultimately, N(SO₂) equals 1.27·10²³.
Where n represents amount of substance.
M refers to molar mass.
Na is Avogadro's number.
Answer:
The molar mass of the gas is 36.25 g/mol.
Explanation:
- To determine this, we utilize the mathematical relationship:
ν = 
Where, ν represents the speed of light in a gas (ν = 449 m/s),
R denotes the universal gas constant (R = 8.314 J/mol.K),
T stands for the temperature of the gas in Kelvin (T = 20 °C + 273 = 293 K),
M is the molar mass of the gas in (Kg/mol).
ν =
(449 m/s) = √(3(8.314 J/mol.K)(293 K)/M,
by squaring both sides:
(449 m/s)² = (3(8.314 J/mol.K)(293 K))/M,
thus M = (3(8.314 J/mol.K)(293 K)/(449 m/s)² = 7308.006/201601 = 0.03625 Kg/mol.
Thus, the molar mass of the gas is 36.25 g/mol.
Answer:
The nichrome wire has contaminants.
The sample solution might be tainted.
Explanation:
If the nichrome wire is contaminated, sodium impurities could be causing the yellow flame. The wire is initially placed in the flame without the sample to check for such impurities.
The testing solution could also be contaminated, causing it to display a color different from the anticipated shade of the test ion.
Answer:
Chemists observe phenomena on a macroscopic level which informs their understanding of microscopic aspects.
Explanation:
Many critical chemical insights arise from macroscopic observations because most scientific instruments currently cannot directly evidence microscopic events. Data gathered from these larger-scale observations can yield valuable insights into the nature of specific microscopic interactions.
This is particularly true in atomic structure studies. The majority of evidence that contributed to our understanding of atomic structure was obtained from macroscopic observations and subsequently provided crucial information regarding the atom's microscopic configuration.
Based on the titration results, the adult would need to consume 85.7 mL to meet the recommended daily intake of 60 mg of Vitamin C. This is calculated from the average total volume of DCPIP used during trials.
