Answer:
The new temperature will be 2546 K or 2273 °C
Explanation:
Step 1: Data given
The initial temperature = 1000 °C =1273 K
The volume = 20L
The volume increases to 40 L
Step 2: Calculate the new temperature
V1/T1 = V2/T2
⇒with V1 = the initial volume = 20L
⇒with T1 = the initial temperature = 1273 K
⇒with V2 = the increased volume = 40L
⇒with T2 = the new temperature = TO BE DETERMINED
20L/ 1273 K = 40L / T2
T2 = 40L / (20L/1273K)
T2 = 2546 K
The new temperature will be 2546 K
This is 2546-273 = 2273 °C
Since the volume is doubled, the temperature is doubled as well
First, you need to have a periodic table that contains the electronegativities values. once you have them, you just need to subtract the values of the atoms and each bond. I have attached a table with these values. also, it does not matter then order in which you subtract them because they are always positive values. even though you get negative values in your calculator, just make it positive.
H-S----> 2.1 - 2.5= 0.4
H-Cl---> 2.1 -3.0=0.9
H-O---> 2.1- 3.5= 1.4
H-F----> 2.1 - 4.0= 1.9
HF is the most polar because it has the highest electronegativity difference.
The last option is correct
Answer:
ΔU = 103.54 KJ
Explanation:
∴ ΔU = Q + W
ideal gas:
∴ PV = nRT
∴ R = 8.314 L.KPa/K.mol
∴ n = 3000 g N2 * ( mol/28.0134g N2) = 107.143 mol N2
∴ m N2 = 3.0 Kg
∴ T1 = 300 K
∴ P1 = 100 KPa
∴ V1 = nRT1/P1 = 2672.36 L = 2.67 m³
⇒ V2 = 0.9*V1 = 2405.12 L = 2.41 m³
∴ P2 = 140 KPa
⇒ T2 = P2.V2/n.R = 377.99 ≅ 378 K
⇒ W = P1V1 - P2V2
⇒ W = ((100KPa)*(2.67m³)) - ((140KPa)*(2.41m³))
⇒ W = - 70.164 KJ
∴ Q = nCpΔT
∴ Cp = (5/2)*R = 20.785 J/mol.K ....ideal gas
⇒ Q = (107.143mol)*(20.785 J/mol.K)*(378 - 300)
⇒ Q = 173703.446 J = 173.703 KJ
⇒ ΔU = 173.703 KJ - 70.164 KJ
⇒ ΔU = 103.54 KJ
For cations, the loss of an electron leaves them with a net positive charge, whereas for anions, the addition of an electron leaves them with a net negative charge. Understanding the processes behind this, including the ionization energy and electron affinity of different atoms, helps you see why certain atoms become ions more easily than others and what causes it to happen.
