Balance Chemical Equation,
2 CO + O₂ → 2CO₂
Acc. to this reaction,
88 g (2 mole) of CO₂ was produced when = 56 g (2 mole)of CO was reacted
So,
24.7 g of CO₂ will be produced by reacting = X g of CO
Solving for X,
X = (56 g × 24.7 g) ÷ 88 g
X = 2.26 g ÷ 88 g
X = 0.0257 g of CO
Result:
0.0257 g of CO is required to be reacted with excess of O₂ to produce 24.7 g of CO₂.
Answer:
High pressure and low temperature, because particles are forced close together and moving slower, so intermolceular forces of attraction increase.
Explanation:
The properties of an ideal gas are explained by the kinetic-molecular theory. An ideal gas assumes there is no intermolecular attraction between the molecules. High pressure would make the particles closer together and interact more, going against the kinetic molecular theory that states there are large spaces between particles and no interactions between particles. Low temperature would make the particles slow which prevents them from overcoming the intermolecular attraction between particles.
QUICK ANSWER
Electrons have a relative mass of 9.1 x 10^-31 kilograms, or 0.51 megaelectron volts. They are a lot smaller than protons and neutrons; and, an electron is roughly 0.054 percent of the mass of one neutron.
Answer:
There are many examples of electrostatic phenomena, from those as simple as the attraction of the plastic wrap to one's hand after it is removed from a package to the apparently spontaneous explosion of grain silos, the damage of electronic components during manufacturing, and photocopier & laser printer operation