Answer:
Aluminum Reacts With Hydrochloric Acid To Produce Aluminum Chloride And Hydrogen Gas. 2Al(s) + 6HCl(aq) -> 2AlCl3(aq) + 3H2(g)What Mass Of H2(g) Is Required From The Reaction Of 0.75 G Of Al(s) With Excess Hydrochloric
Answer:
kilopascal, torr, and atmosphere
Explanation:
There is 18.4 % oxygen in the compound, 12.8 % hydrogen in the compound and 69.0 % carbon in the compound.
The molecular formula of the compound is; C10H22O2. From this, we can calculate the molar mass of the compound as follows;
Molar mass = 10(12) + 22(1) + 2(16) = 120 + 22 + 32 = 174 g
Percent of oxygen in the compound = 32.00 g/174 g × 100/1 = 18.4 %
Percent of hydrogen in the compound = 22.22 g/174 g × 100/1 = 12.8 %
Percent of carbon in the compound = 120.10 g/174 g × 100/1 = 69.0 %
Hence, there is 18.4 % oxygen in the compound, 12.8 % hydrogen in the compound and 69.0 % carbon in the compound.
Learn more: brainly.com/question/19580143
Answer:
9.59 atm
Explanation:
Use ideal gas law PV = n RT
V = 5.34 L n = 1.82 mole T = ( 69.58+ 273.15) = 342.73 K
R = .082057 L-Atm/(K - mole)
P = n RT / V = 9.59 Atm
that' the answer i don't need an explanation
