All three phases can exist in an equilibrium with one another at the __ of a substance
1 answer:
Answer:
Triple point
Explanation:
Yes, all three phases can exist in an equilibrium with one another at the triple point of a substance.
In thermodynamics, the triple point of a substance is defined as the point at which all three phases of substance co-exist together at a particular pressure and temperature.
for example, the triple point of mercury occurs at a temperature of −38.83440 °C and a pressure of 0.2 mPa.
And for water it is 0.01 °C and 611.73 pascals.
you will get some clear idea after seeing the graph.
And critical point as you see in the graph is end point of phase equilibrium curve, mainly liquid-vapor equilibrium
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Answer:
Explanation:
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In this case, since the ionization of ammonia, which is a weak base, is written as:
We can see that the ammonium ion is the conjugate acid whereas the hydroxide ions the conjugate base; that is why we use the Henderson-Hasselbach equation to compute the pH, given the pKb of ammonia 4.75:
In such a way, for the given moles of ammonia, base, and those of ammonium chloride, conjugate acid form, we obtain:
Best regards!
An acid is a compound which will give H+ ions or H3O^+ ions
the reaction will be
Thus as there is evolution of H_{3}O^{+} the Mn+3 is an acid
Answer:
1.69 g Na₂O
General Formulas and Concepts:
<u>Chemistry - Atomic Structure</u>
- Reading a Periodic Table
- Using Dimensional Analysis
Explanation:
<u>Step 1: Define</u>
0.0273 mol Na₂O
<u>Step 2: Identify Conversions</u>
Molar Mass of Na - 22.99 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of Na₂O - 2(22.99) + 16.00 = 61.98 g/mol
<u>Step 3: Convert</u>
<u /> = 1.69205 g Na₂O
<u>Step 4: Check</u>
<em>We are given 3 sig figs. Follow sig fig rules and round.</em>
1.69205 g Na₂O ≈ 1.69 g Na₂O