Answer:
6.9 ml of concentrate
Explanation:
100 ml of .1 M will require .01 moles
from a 1.45 M solution, .01 mole would be
.01 mole / ( 1.45 mole / liter) = 6.9 ml of the concentrate then dilute to 100 ml
Answer:
1. d[H₂O₂]/dt = -6.6 × 10⁻³ mol·L⁻¹s⁻¹; d[H₂O]/dt = 6.6 × 10⁻³ mol·L⁻¹s⁻¹
2. 0.58 mol
Explanation:
1.Given ΔO₂/Δt…
2H₂O₂ ⟶ 2H₂O + O₂
-½d[H₂O₂]/dt = +½d[H₂O]/dt = d[O₂]/dt
d[H₂O₂]/dt = -2d[O₂]/dt = -2 × 3.3 × 10⁻³ mol·L⁻¹s⁻¹ = -6.6 × 10⁻³mol·L⁻¹s⁻¹
d[H₂O]/dt = 2d[O₂]/dt = 2 × 3.3 × 10⁻³ mol·L⁻¹s⁻¹ = 6.6 × 10⁻³mol·L⁻¹s⁻¹
2. Moles of O₂
(a) Initial moles of H₂O₂

(b) Final moles of H₂O₂
The concentration of H₂O₂ has dropped to 0.22 mol·L⁻¹.

(c) Moles of H₂O₂ reacted
Moles reacted = 1.5 mol - 0.33 mol = 1.17 mol
(d) Moles of O₂ formed

Answer:
C co2 2co enthalpy
2 Answers. Ernest Z. The standard enthalpy of formation of carbon monoxide is -99 kJ/mol.
Unrestricted populations of organisms experience Exponential growth.
As a population reaches is carrying capacity there is an increase in competition for All of the above.
Hope I helped.