I've put in some of the answers.
hope this helps :)
Answer: Molar mass of thyroxine is 776.5 g/mol.
Explanation:
Mass of thyroxine = 0.455 g
Mass of benzene = 10g =0.01kg (1 kg = 1000 g)
Formula used :
where,
= change in freezing point =
= freezing point constant =
m = molality
Now put all the given values in this formula, we get
Thus molar mass of thyroxine is 776.5 g/mol.
Answer:
n = 2 moles (1 sig-fig)
Explanation:
Using the Ideal Gas Law equation (PV = nRT), solve for n (= moles) and substitute data for ...
pressure = P(atm) = 100atm
volume =V(liters) = 50L
gas constant = R = 0.08206L·atm/mol·K
temperature = T(Kelvin) = °C + 273 = (35 + 273)K = 308K
PV = nRT => n = PV/RT = (100atm)(50L)/(0.08206L·atm/mol·K)(308K)
∴ n(moles) = 1.978moles ≅ 2 moles gas (1 sig-fig) per volume data (= 50L) that has only 1 sig-fig. (Rule => for multiplication & division computations round final answer to the measured data having the least number of sig-figs).
If a compound is made of one metal and one non-metal it's bond will be ionic, whereas if a compound is made of two non-metals, it's bond will be covalent.
C - Non-Metal
O - Non-Metal
CO = Covalent.
Answer:
0.5 mole
Explanation:
The question isn't even clear
But I'm guessing you want to ask the number of moles
n= Number of molecules/ Avogadros number
n= 1/2