Answer:
Approximately 
, assuming that all sulfur in that coal was converted to 
.
Explanation:
Look up the relative atomic mass of 
and 
on a modern periodic table:
Convert the unit of the mass of coal to grams:
.
Mass of sulfur in that much coal:
.
The relative atomic mass of sulfur is 
. Therefore, the mass of each mole of sulfur atoms would be 
. Calculate the number of moles of atoms in that 
of sulfur:
.
Each 
molecule contains one sulfur atom. Therefore, assuming that all those (approximately) 
of sulfur atoms were converted to molecules through the reaction with 
, (approximately) 
of 
molecules would be produced.
Calculate the mass of one mole of molecules:
.
The mass of that of molecules would be:
.
The characteristic being calculated here is the mean or the average of the data set.
To check:
(20.73 + 20.76 + 20.68 + 20.75)/4 [we divide it by 4 because there are 4 numbers]
= 82.92 / 4
= 20.73
Answer:
δ N2(g) = 1.1825 g/L
Explanation:
- δ ≡ m/v
- Mw N2(g) = 28.0134 g/mol
ideal gas:
∴ P = (837 torr)×( atm/760 torr) = 1.1013 atm
∴ T = 45.0 °C + 273.15 = 318.15 K
∴ R = 0.082 atm.L/K.mol
⇒ n/V = P/R.T
⇒ n/V = (1.1013 atm) / ((0.082 atm.L/K.mol)(318.15 k))
⇒ n/V = 0.0422 mol/L
⇒ δ N2(g) = (0.042 mol/L)×(28.0134 g/mol) = 1.1825 g/L
Frequency of photon = is 6.85 X 10¹⁴ sec⁻¹
Energy of photon , E = hv
where h is Planck's constant, v is the frequency of photon
E = 6.63 × 10⁻³⁴ J.s x 6.85 X 10¹⁴ s⁻¹
E = 4.54 x 10⁻¹⁹ J
Therefore, the energy of a photon of green light is 4.54 x 10⁻¹⁹ J.
.