To find the temperature in the problem, we apply the ideal gas law, PV=nRT where R=8.314 Pam3/mol K. Substituting the given, T= 153,000 Pa*1.5x10^-4 m3/ [(0.75 mol)(<span>8.314 Pam3/mol K)]. The temperature is equal to 3.68 kelvin. </span>
Answer:
The molarity is 0.203 M
Explanation:
Using the formula C(oxi) x V(oxi) / [C(red) x V(red)] = N(oxi) / N(red)
Where oxi and red means reducing agent and oxidising agent respectively.
C = Concentration, V = Volume and N = number of moles.
C(oxi) = 0.5 M
V(oxi) = mL
C(red) = ?
V(red) = 30mL
Equation of reaction = 2K2S2O3 + KI3 = K2S4O6 + 3KI
so N(red) = 1 , N(oxi) = 2
from the equation above,
C(red) = 0.5 x 25 x 1 / (2 x 30)
= 0.203 M.
Answer:
151.94 u
Explanation:
The atomic mass of Eu is the <em>weighted average</em> of the atomic masses of its isotopes.
We multiply the atomic mass of each isotope by a number representing its relative importance (i.e., its <em>percent abundance</em>).
The atomic masses of Eu-151 and Eu-153 are 150.92 u and 152.92 u, respectively.
Set up a table for easy calculation.
0.4803 × 150.92 u = 72.472 u
0.5197 × 152.92 u = <u> 79.473 u
</u>
TOTAL = 151.94 u
Answer:
D.
Explanation:
I took this test as a freshman and this was the only question of 4 that I can remember
