Answer:
The answer is 1.15m.
Since molality is defined as moles of solute divided by kg of solvent, we need to calculated the moles of H2SO4 and the mass of the solvent, which I presume is water.
We can find the number of H2SO4 moles by using its molarity
C=nV→nH2SO4=C⋅VH2SO4=6.00molesL⋅48.0⋅10−3L=0.288
Since water has a density of 1.00kgL, the mass of solvent is
m=ρ⋅Vwater=1.00kgL⋅0.250L=0.250 kg
Therefore, molality is
m=nmass.solvent=0.288moles0.250kg=1.15m
Molar mass = 305.42 g/mol
C = ( 12 x 18 / 305.42 ) x 100 => 70.72 % of C
H = ( 1 x 27 / 305.42 ) x 100 => 8.84 % of H
N = ( 14 x 1 / 305.42 ) x 100 => 4.58 % of N
O = ( 16 x 3 / 305.42) x 100 => 15.71% of O
hope this helps!
Answer:
186 Liters at STP conditions
Explanation:
1 mole of any gas at STP conditions occupies 22.4 Liters.
Therefore, 8.32 moles O₂(g) = 8.32 moles x 22.4Liters/mole = 186 Liters (3 sig.figs.)
Answer:
a
Explanation
Bc I took the test, good luck with that guys
