I don’t know so ask someone else
H2O2(I)
C6H6(O)
CO2(I)
C2H6(O)
HNO3(I)
Answer:
Explanation:
Combustion can be defined as the burning of a compound in the presence of oxygen to produce carbon dioxide and water. Because it involves the release of heat (energy), it is referred to as an exothermic reaction.
Fuel is an <u>organic compound</u> and it's combustion will also go through the process above and also <u>releases heat (exothermic reaction)</u> into the atmosphere after burning. However, same can be said about forest fire also; as the forest is made up of plants (whose major <u>constituents are organic </u>also). The forest fire can also be termed as combustion because it burns in the presence of oxygen, <u>releasing heat (energy) into the atmosphere</u> (which also makes it an <u>exothermic reaction</u>).
Answer:
m = 0.3249 g
Explanation:
First, I'm assuming you have a reaction of mercury(II) oxyde descomposition. If this is the case, then the equation to use is the following:
HgO ---------> Hg + O2
Balancing the equation:
2HgO ----------> 2Hg + O2
This means that 2 moles of HgO reacts to produce 1 mole of O2, so, we first calculate the moles of O2, then, the moles of HgO and finally the mass:
We have the volume of O2, the pressure and temperature, so let's use the ideal gas equation:
PV = nRT
Solving for n:
n = PV/RT
R: 0.082 L atm / K mole
T = 70 + 273 = 343 K
V = 83 / 1000 = 0.083 L
Calculating n:
n = 1 * 0.083 / 0.082 * 343
n = 0.003 moles
as stated before, 2 moles of HgO reacts with 1 mole of oxygen so:
2 moles HgO = 1 moles O2
moles HgO = moles O2 / 2
moles HgO = 0.003 / 2 = 0.0015 moles
Finally, to calculate the mass:
m = n * MM
the molar mass of HgO is 216.59 g/mol, so replacing:
m = 0.0015 * 216.59
m = 0.3249 g
Answer:
The spectroscope scale is illuminated so that one can know exactly where the wavelengths of the lines are falling along.