The average molar mass of an atom is equal to the summation of the molar mass of the isotopes multiplied by their relative abundance. In this case, we substitute and use the formula:
MW ave = 49.946044 amu*0.04345 + <span>51.940508 amu * 0.83789 + </span><span> 52.940649 amu * 0.09501 + </span><span>53.93880 amu * 0.02365 = 51.966 amu.
Answer is C</span>
To balance the chemical reaction above, we need to remember that the amount of the elements in the reactant side should be equal to the amount of that element in the product side. The balanced chemical reaction is written as:
<span>N2O5 +H2O --->2HNO3</span>
in order for a scientific theory to become a scientific law it needs to be tested with generations of data to confirm that it is really true.
Q = m. C. ΔT
Δt = Δf - Δi = 49.0 - 24.0 = 25ºC
C = Q / m . ΔT
C = 468.2 / 80.0 . 25
C = 468.2 / 2000
C = 0.2341 J/gºC
hope this helps!
Answer:
0.488 mol
Explanation:
By the ideal gas law:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.082 atm.L/mol.K), and T is the temperature in K. Thus, after the reaction:
P = 2.92 atm
V = 4.50 L
T = 55.2°C + 273 = 328.2 K
PV = nRT
n = PV/RT
n = (2.92*4.50)/(0.082*328.2)
n = 0.488 mol