Compact fluorescent bulbs because they made out of glass that will break and will dye and then they can't be used again
Answer:
B) C3H3O and C6H6O2
Explanation:
Given data:
Molar mass of compound = 100 g/mol
Percentage of hydrogen = 5.45%
Percentage of carbon = 65.45%
Percentage of oxygen = 29.09%
Empirical formula = ?
Molecular formula = ?
Solution:
Number of gram atoms of H = 5.45 / 1.01 = 5.4
Number of gram atoms of O = 29.09/ 16 = 1.8
Number of gram atoms of C = 65.45 / 12 = 5.5
Atomic ratio:
C : H : O
5.5/1.8 : 5.4/1.8 : 1.8/1.8
3 : 3 : 1
C : H : O = 3 : 3 : 1
Empirical formula is C₃H₃O.
Molecular formula:
Molecular formula = n (empirical formula)
n = molar mass of compound / empirical formula mass
Empirical formula mass = 12×3 + 1.01 ×3 + 16×1 = 55.03
n = 100 / 5503
n = 2
Molecular formula = n (empirical formula)
Molecular formula = 2 (C₃H₃O)
Molecular formula = C₆H₆O₂
The answer is B hope this is right
Answer: The pressure will be equal to 0.19 atm.
Explanation:
The Ideal Gas Equation states the relationship among the pressure, temperature, volume, and number of moles of a gas.
The equation is:

where P = pressure in <em>atm</em>
V = volume in <em>L</em>
n = numbers of moles of gas in <em>mol</em>
R = universal gas constant = 0.08206 
T = temperature in <em>K</em>
Based on the problem,
mass of O2 = 1.0 g
V = 4.00 L
T = 293 K
mol of O2 = ?
P = ?
We need to calculate the moles of O2 before we can use the Ideal Gas Equation. To solve the number of moles, we use the equation:

The molar mass of O2 is 32 g/mol, therefore,

no. of moles of O2 = 0.03125 mol.
Now we substitute the values into the Ideal Gas equation:

Solving for P, we will get

In correct significant figures, P is equal to 0.19 atm.