At standard temperature and pressure, it is established that 1 mole of gas has a volume of 22.4 liters.
According to the periodic table:
the molar mass of oxygen is 16 g
and the molar mass of hydrogen is 1 g
Hence, the molar mass of water vapor is calculated as 2(1) + 16 = 18 g
Thus, 18 g of water occupies 22.4 liters, therefore:
the volume for 32.7 g is (32.7 x 22.4) / 18 = 40.6933 liters
Laws of Nature should be differentiated from Scientific and Natural Laws. The Necessitarian Theory suggests that Laws of Nature are those principles which influence the natural phenomena in the universe, meaning the natural world adheres to them.
The enthalpy change in this scenario totals 7.205 KJ. The task is to compute the enthalpy variation during the conversion of 10.0 g of ice at -25.0°C into water at 80.0°C, factoring in specific heats and enthalpy for phase transitions.
The reaction will yield 2 mol of H₂O. The balanced chemical equation for this process is: c3h8 (g) + 5o2 (g) → 3co2 (g) + 4h2o (g). Since 5 moles of O₂ create 4 moles of H₂O, 2.5 mol of O₂ will produce: 2.5 x 4/5 = 2 mol of H₂O.
The molar masses for H2S and NH3 are 34 and 17 g/mol, respectively. The appropriate equation to represent this is,
Rate A/Rate B = √(molar mass B/molar mass A)
Substituting values,
x/77 = √(17 /34 )
x = 54.4
This means NH3 will take 54.4 seconds to escape through the container.
