Answer:
[KI] = 0.17 M
Explanation:
We determine the moles of solute:
Mass / Molar mass → 4.73 g / 166 g/mol = 0.0285 moles
Molarity (mol/L) is defined as moles of solute in 1L of solution
It is a sort of concentration
M = 0.0285 mol / 0.169L = 0.17 M
Instead of making the division (mol/L), we can also try this rule of three:
In 0.169 L we have 0.0285 moles of solute
in 1 L we must have ___ (1 . 0.0285) / 0.169 = 0.17 mol/L
Answer:
the percent error is -13.5%
Explanation:
Given the data in the question;
Exact atomic weight = 65.38 g/mol
For approx
increased mass = 0.3681 g
moles = 6.514 x 10⁻³
we know that; moles = mass / (Atomic mass )
so
Atomic mass_
= mass / moles
Atomic mass_
= 0.3681 / 6.514 x 10⁻³
Atomic mass_
= 56.509
so approx atomic weight = 56.51 g/mol
we know that;
% error = ( [approx - exact] / exact ) × 100
we substitute
% error = ( [56.51 - 65.38] / 65.38 ) × 100
% error = (-8.87 / 65.38 ) × 100
% error = ( -0.1356684 ) × 100
% error = -13.5%
Therefore, the percent error is -13.5%
The are isotopes because the atomic number (meaning a same number of protons) is the same but the atomic masses are different. this means they have a different number of neutrons which is what isotopes are.
answer is E- all of these
V₁/T₁ = V₂/T₂ = const
T₁=11+273=284K
V₂=3V₁
V₁/T₁=3V₁/T₂
T₂=3T₁
T₂=3*284=852K
t₂=852-273=579°C