Um for this question it is all about your beliefes and how you view them.
Answer:
halogens
Explanation:
Elements that are nonmetals tend to gain electrons and become negatively charged ions called anions
Answer:
The parcial pressure of N₂ in the mixture is 1.24 atm.
Explanation:
The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:
PT = PA + PB
This relationship is due to the assumption that there are no attractive forces between the gases.
In this case:
PT=PHe + PNe + PN₂
You know:
- PT= 1.943 atm
- PHe= 0.137 atm
- PNe= 0.566 atm
- PN₂= ?
Replacing:
1.943 atm= 0.137 atm + 0.566 atm + PN₂
Solving:
1.943 atm= 0.703 atm + PN₂
1.943 atm - 0.703 atm= PN₂
1.24 atm= PN₂
<u><em>The parcial pressure of N₂ in the mixture is 1.24 atm.</em></u>
The answer:
La planta tiene las hojas secas.
Using the ideal gas law equation, we can find the number of H₂ moles produced.
PV = nRT
Where P - pressure - 0.811 atm x 101 325 Pa/atm = 82 175 Pa
V - volume - 58.0 x 10⁻³ m³
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature - 32 °C + 273 = 305 K
substituting these values in the equation,
82 175 Pa x 58.0 x 10⁻³ m³ = n x 8.314 Jmol⁻¹K⁻¹ x 305 K
n = 1.88 mol
The balanced equation for the reaction is as follows;
CaH₂(s) + 2H₂O(l) --> Ca(OH)₂(aq) + 2H₂(g)
stoichiometry of CaH₂ to H₂ is 1:2
When 1.88 mol of H₂ is formed , number of CaH₂ moles reacted = 1.88/2 mol
therefore number of CaH₂ moles reacted = 0.94 mol
Mass of CaH₂ reacted - 0.94 mol x 42 g/mol = 39.48 g of CaH₂ are needed
