Answer:
Indeed, the chemist is capable of identifying the compound present in the sample.
Explanation:
In one mole of K₂O, potassium has a mass of 2 × 39.1 g = 78.2 g, while the total mass of K₂O is 94.2 g. The mass ratio of K compared to K₂O is calculated as 78.2 g / 94.2 g = 0.830.
For 1 mole of K₂O₂, potassium's mass remains the same at 78.2 g, but the total mass of K₂O₂ is 110.2 g. The mass ratio of K to K₂O₂ then equates to 78.2 g / 110.2 g = 0.710.
When the chemist measures the mass of K in relation to the overall sample, the mass ratio can be computed.
- If the mass ratio is 0.830, then it indicates a pure K₂O compound.
- If the mass ratio is 0.710, it indicates a pure K₂O₂ compound.
- If the mass ratio falls outside of 0.830 or 0.710, the sample is assessed to be a mixture.
Answer: Option (a) is the correct answer.
Explanation:
Under conditions of low pressure and high temperature, gas molecules exhibit negligible attractions or repulsions among themselves. Hence, gases behave ideally in these scenarios.
Conversely, at low temperatures, there is a reduction in the kinetic energy of gas molecules, while high pressure compels the molecules to be closer together.
Thus, attractive forces emerge between molecules in conditions of low temperature and high pressure, causing gases to be termed real gases.
Therefore, we conclude that the ideal gas law becomes less accurate when pressure increases and temperature decreases.
1) To find the molar mass of C6H8O6, you must refer to the atomic weights of C, H, and O from the periodic table: C is 12; H is 1; O is 16 <span> (12x6)+(1x8)+(16x6)= 176g/mol
</span> <span> 176 g = 1 mol
0.5 g = x mol = 500 mg = 0.5 grams
Molar mass = mass ÷ moles
176 = 0.5 ÷ x
x = 2.84 x 10⁻³ mol
2) To calculate the total number of molecules in those </span> 2.84 x 10⁻³ mol, multiply the moles by <span> Avogadro's constant.
Number of molecules = Avogadro's constant x number of moles
Number of molecules = 6.022 x 10²³ x 2.84 x 10⁻³ </span> = 1.71 x 10²¹ molecules of vitamin C. <span>
</span>
Answer:
The ratios arranged in ascending order are; The ratio of the mass of Y to X in XY2 divided by the mass of Y to X in XY, The ratio of the mass of Y to X in XY3 divided by the mass of Y to X in XY, The ratio of the mass of Y to X in XY4 divided by the mass of Y to X in XY
1) Mass ratio = 3
2) Mass ratio = 2
3) Mass ratio = 4
Explanation:
Comprehensive calculations are displayed in the attachment.
Answer:
The temperature increase of the calorimeter, which is missing in the problem, is necessary for the calculation.
Explanation:
Since the temperature rise (X) is unspecified, we'll express the calculation in terms of X, and demonstrate with an example value.
1) Calorimeter details:
- Temperature increase: X °C
- Heat capacity ratio: 4.87 J / 5.5 °C (given)
- Energy absorbed by calorimeter at X °C rise:
(4.87 J / 5.5 °C) × X
2) Reaction data:
- Heat released: 362 kJ per mole of reactant
- Number of moles consumed: n
- Total energy from reaction:
362 kJ/mol × 1000 J/kJ × n = 362,000 n J
3) Using energy conservation, assuming no heat loss to surroundings, the energy from the reaction equals the energy absorbed by the calorimeter:
- 362,000 n = (4.87 J / 5.5 °C) × X
- n = [(4.87 / 5.5) × X] / 362,000
n = 0.000002446 × X
This means for each degree Celsius rise in calorimeter temperature, 0.000002446 moles of reactant were consumed.
Example:
If the calorimeter temperature increases by 100 °C, then:
- n = 0.000002446 × 100 = 0.0002446 mol
