It's a replacement reaction. Hope it helped
Answer:
The van't Hoff factor = 3.20
Explanation:
Step 1: data given
Osmotic pressure of a 0.050 M Solution is 3.85 atm
Temperature = 20.0 °C
Step 2:
Osmotic pressure depends on the molar concentration of the solute but not on its identity.
We can calculate the osmotic pressure by:
π = i.M.R.T
⇒ with π = osmotic pressure = 3.85 atm
⇒ with i = van 't Hoff factor = TO BE DETERMINED
⇒ with M = molar concentration of the solution =0.050 M
⇒ with R = gas constant =0.08206 L * atm / mol* K)
⇒ with T = Temperature of the solution =20°C = 293 K
i = π / M.R.T
i = 3.85 / 0.050*0.08206*293
i = 3.20
The theoretical Van't Hoff factor is 4:
AlCl3(aq) → Al^3+(aq) + 3Cl^-(aq)
AlCl3 dissociates in 1 mol Al^3+ + 3 moles Cl-
Due to the interionic atractions the Van't hoff factor is less than the theoretical value of 4
B. 6 atoms of carbon C
I would think this is the answer, because one can't just delete or add atoms; otherwise, the equation would be unbalanced. This also abides with the Law of Conservation of Mass.
Plus, I also came to that conclusion because if we look at the net equation of photosynthesis:
––>
The number of Carbon atoms is 6 on both the reagent's side and the product's side.
Answer:
The change in internal energy is - 1.19 kJ
Explanation:
<u>Step 1:</u> Data given
Heat released = 3.5 kJ
Volume calorimeter = 0.200 L
Heat release results in a 7.32 °C
Temperature rise for the next experiment = 2.49 °C
<u>Step 2:</u> Calculate Ccalorimeter
Qcal = ccal * ΔT ⇒ 3.50 kJ = Ccal *7.32 °C
Ccal = 3.50 kJ /7.32 °C = 0.478 kJ/°C
<u>Step 3:</u> Calculate energy released
Qcal = 0.478 kJ/°C *2.49 °C = 1.19 kJ
<u>Step 4:</u> Calculate change in internal energy
ΔU = Q + W W = 0 (no expansion)
Qreac = -Qcal = - 1.19 kJ
ΔU = - 1.19 kJ
The change in internal energy is - 1.19 kJ
Answer: 12.011g/mol
Explanation: The molar mass of any element is usually stated at the bottom of periodic table (depending of your table anyways). Remember that the periodic table speaks to you in moles so every molar mass under the element is for 1 mole. By this I mean for example, 1 mole of Carbon = 12.011g of Carbon.
