<h3>
Answer:</h3>
The equation is; P₁V₁/T₁ = P₂V₂/T₂
<h3>
Explanation:</h3>
Concept being tested: Combined gas law
We need to know the two gas laws that form the combined gas law
- The combined gas laws is derived from the Boyle's gas law and Charles's law.
- According to Boyle's law;
P₁V₁ = P₂V₂
- On the other hard, according to Charles's law;
V₁/T₁= V₂/T₂
- The combine gas laws combines both Boyle's law and Charles's law.
- According to the combined gas law, the volume of a fixed mass of a gas i inversely proportional to pressure and directly proportional to its absolute temperature.
- Therefore, combining both Boyle's law and Charles's law, we get;
P₁V₁/T₁ = P₂V₂/T₂
- Thus, based on Combined gas law, then
P₁V₁/T₁ = P₂V₂/T₂
Answer:
Q₁- The concentration of HCl = 0.075 N = 0.075 M.
Q₂- The concentration of KOH = 7.675 mN = 7.675 mM.
Q₃- The concentration of H₂SO₄ = 0.2115 N = 0.105 M.
Q₄- The equivalence point is the point at which the added titrant is chemically equivalent completely to the analyte in the sample whereas the endpoint is the point where the indicator changes its color.
Explanation:
<u><em>Q₁:
</em></u>
- As acid neutralizes the base, the no. of gram equivalent of the acid is equal to that of the base.
- The normality of the NaOH and HCl = Their molarity.
∵ (NV)NaOH = (NV)HCl
∴ N of HCl = (NV)NaOH / (V)HCl = (0.15 N)(67 mL) / (134 mL) = 0.075 N.
∴ The concentration of HCl = 0.075 N = 0.075 M.
<em><u>Q₂:</u></em>
- As mentioned in Q1, the no. of gram equivalent of the acid is equal to that of the base at neutralization.
- The normality of H₂SO₄ = Molarity of H₂SO₄ x 2 = 0.050 M x 2 = 0.1 N.
∵ (NV)H₂SO₄ = (NV)KOH
∴ N of KOH = (NV)H₂SO₄ / (V)KOH = (0.1 N)(27.4 mL) / (357 mL) = 7.675 x 10⁻³ N = 7.675 mN.
∴ The concentration of KOH = 7.675 mN = 7.675 mM.
<em><u>Q₃:</u></em>
- As mentioned in Q1 and 2, the no. of gram equivalent of the acid is equal to that of the base at neutralization.
- The normality of NaOH = Molarity of NaOH = 0.5 N.
∵ (NV)H₂SO₄ = (NV)NaOH
∴ N of H₂SO₄ = (NV)NaOH / (V)H₂SO₄ = (0.5 N)(55 mL) / (130 mL) = 0.2115 N.
∴ The concentration of H₂SO₄ = 0.2115 N = 0.105 M.
<em><u>Q₄:</u></em>
- The equivalence point is the point at which the added titrant is chemically equivalent completely to the analyte in the sample whereas the endpoint is the point where the indicator changes its color.
- The equivalence point in a titration is the point at which the added titrant is chemically equivalent completely to the analyte in the sample. It comes before the end point. At the equivalence point, the millimoles of acid are chemically equivalent to the millimoles of base.
- End point is the point where the indicator changes its color. It is the point of completion of the reaction between two solutions.
- The effectiveness of the titration is measure by the close matching between equivalent point and the end point. pH of the indicator should match the pH at the equivalence to get the same equivalent point as the end point.
<span>MgO + HCl = MgCl2* + H2*O
To balance an equation, you have to have both the reactants and products side equal.
Mg = 1 Mg = 1
H = 1 H = 2
Cl = 1 Cl = 2
MgO + 2HCl = MgCl2 + H2*O
We added the coefficient 2, so they could balance. </span>
Answer:
When an atom is in an excited state, the electron can drop all the way to the ground state in one go, or stop on the way in an intermediate level. Electrons do not stay in excited states for very long - they soon return to their ground states, emitting a photon with the same energy as the one that was absorbed.
HOPE IT HELPS
I know CL is chlorine and NA is sodium.
