Answer:
Yes, it underwent a chemical change
Explanation:
The average atomic mass of hydrogen (99% H-1, 0.8% H-2, and 0.2% H-3) is 1.012 amu.
The average atomic mass of hydrogen can be calculated with the following equation:
Where:
: is the mass of protium (H-1) = 1
: is the <em>mass</em> of deuterium (H-2) = 2
: is the <em>mass </em>of tritium (H-3) = 3
: is the abundance percent of H-1 = 99%
: is the <em>abundance percent</em> of H-2 = 0.8%
: is the <em>abundance percent</em> of H-3 = 0.2%
The average atomic mass is:
Changing all the <u>percent values</u> into <u>decimal ones</u>, we have:
Therefore, the average atomic mass of hydrogen is 1.012 amu.
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The balanced equation for the above neutralisation reaction is as follows;
2KOH + H₂SO₄ --> K₂SO₄ + 2H₂O
stoichiometry of KOH to H₂SO₄ is 2:1
neutralisation is the reaction between H⁺ ions and OH⁻ ions to form water which is neutral
number of KOH moles - 1.56 mol
2 mol of KOH require 1 mol of H₂SO₄ for neutralisation
therefore 1.56 mol of KOH require - 1/2 x 1.56 mol = 0.78 mol
0.78 mol of H₂SO₄ are required for neutralisation
Answer:
1.7 atm
Explanation:
For first syringe :
Pressure = 1.2 atm
Temperature = 325 K
Volume = 589 mL = 0.589 L (1 mL = 0.001 L)
Using ideal gas equation as:
PV=nRT
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
1.2 atm × 0.589 L = n × 0.0821 L.atm/K.mol × 325 K
⇒n = 0.02649 moles
For second syringe :
Pressure = 2.6 atm
Temperature = 298 K
Volume = 473 mL = 0.473 L (1 mL = 0.001 L)
Using ideal gas equation as:
PV=nRT
Applying the equation as:
2.6 atm × 0.473 L = n × 0.0821 L.atm/K.mol × 298 K
⇒n = 0.050266 moles
Total moles = 0.02649 moles + 0.050266 moles = 0.076756 moles
Volume = 1 L
Temperature = 0.00 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (0 + 273.15) K = 273.15 K
Using ideal gas equation as:
PV=nRT
Applying the equation as:
P × 1 L = 0.076756 × 0.0821 L.atm/K.mol × 273.15 K
⇒Total P = 1.7 atm