<span>283.89 g/mol is the molar mass of tetraphosphorus decoxide</span>
Answer: 1.99 x 10²² molecules H2
Explanation:First we will solve for the moles of H2 using Ideal gas law PV= nRT then derive for moles ( n ).
At STP, pressure is equal to 1 atm and Temperature is 273 K.
Convert volume in mL to L:
750 mL x 1 L / 1000 mL
= 0.75 mL
n = PV/ RT
= 1 atm ( 0.75 L ) / 0.0821 L.atm/ mole.K ( 273 K)
= 3.3x10-² moles H2
Convert moles of H2 to atoms using Avogadro's Number.
3.3x10-² moles H2/ 6.022x10²³ atoms H2 / 1 mole H2
= 1.99x10²² atoms H2
The first one is the correct answer: <span>The potential energy of the products is greater than that of the reactants and the change in enthalpy is positive.<span> </span></span>
Answer:
Non-metals
Explanation:
Covalent bonds usually occur between nonmetals. For example, in water (H2O) each hydrogen (H) and oxygen (O) share a pair of electrons to make a molecule of two hydrogen atoms single bonded to a single oxygen atom.
How many electrons does each element have to lose again to achieve a noble gas electron configuration?
Answer:
Explanation:
Each element will gain or lose electron to attain the octet of the noble gases in their outer shell electrons.
- Most metals in group 1 and 2 will lose 1 and 2 electrons apiece to attain a noble configuration.
- Non-metals are typically electronegative and will gain considerable amount of electrons to complete their octet.
- Halogens will need one electron to complete their own out shell configuration.
Elements will gain or lose an amount of electron that will make it resemble noble gases.
