Answer:
C₅H₁₀O₄
Explanation:
The empirical formula is the simplest whole-number ratio of atoms in a compound.
The ratio of atoms is the same as the ratio of moles.
So, our job is to calculate the molar ratio of C:H:O.
Assume 100 g of deoxyribose.
1. Calculate the mass of each element.
Then we have 44.8 g C, 7.5 g H, and 47.7 g O.
2. Calculate the moles of each element
3. Calculate the molar ratio of the elements
Divide each number by the smallest number of moles
C:H:O = 3.730:7.44:2.981 = 1.251:2.50:1 = 5.005:9.98:4 ≈ 5:10:4
4. Write the empirical formula
EF = C₅H₁₀O₄
Answer:
56.8cm³
Explanation:
Given parameters:
Measured volume = 54.5cm³
Percentage error = 4.25%
Unknown:
Actual volume of the cylinder = ?
Solution:
The percentage error shows the amount of error introduced into a measurement.
We need to find out this amount of error from the data given.
Error = Percentage error x measured volume
Error = 
x 54.5 = ±2.32cm³
Since the error introduced = 2.32cm³
Actual volume of cylinder = measured volume ± Error
Since the percentage error quoted as higher 4.25%;
Actual volume = 54.5cm³ + 2.32cm³ = 56.8cm³
Answer:
Their answers must be in two decimal places
The problem is incomplete. However, there can only be two probable questions for this problem. First, you can be asked the individual partial pressures of each gas. Second, you can be asked the volume occupied by each gas. I can answer both cases for you.
1.
Let's assume ideal gas.
Pressure for N₂: 2 bar*0.4 = 0.8 bar
Pressure for CO₂: 2 bar*0.5 = 1 bar
Pressure for CH₄: 2 bar*0.1 = 0.2 bar
2. For the volume, let's find the total volume first.
V = nRT/P = (1 mol)(8.314 J/mol-K)(30 +273 K)/(2 bar*10⁵ Pa/1 bar)
V = 0.0126 m³
Hence,
Volume for N₂: 0.0126 bar*0.4 = 0.00504 m³
Volume for CO₂: 0.0126*0.5 = 0.0063 m³
Volume for CH₄: 0.0126*0.1 = 0.00126 m³
