Answer:
T₂ = 506.6 K
Explanation:
Given data:
Initial pressure of gas = 25°C (25+273 =298 K)
Initial temperature = 0.500 atm
Final pressure = 0.850 atm
Final temperature = ?
Solution:
According to Gay-Lussac Law,
The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.
Mathematical relationship:
P₁/T₁ = P₂/T₂
Now we will put the values in formula:
0.500 atm / 298 K = 0.850 atm /T₂
T₂ = 0.850 atm × 298 K / 0.500 atm
T₂ = 253.3 atm. K / 0.500 atm
T₂ = 506.6 K
In the first shell there is 2 electrons and on the second shell there is 4 elections.
x=3
Use the pythagorean theorem:
a^2 + b^2 = c^2
4^2 + x^2 = 5^2
16 + x^2 = 25
x^2 = 25-16
x^2 = 9
√x^2 = √9
x = 3
Hey there!
Compounds with ionic bonds have higher melting points because of the forces needed to break through the strong forces of attraction holding it together.
Compounds with covalent bonds have lower melting points because less energy is needed to break the weaker forces of attraction.
So, your answer is C. Compound 1 is ionic, and compound 2 is molecular.
Hope this helps!
