P x V = n x R x T
1.00 x V = 3.50 x 0.082 x 273
1.00 x V = 78.351
V = 78.351 / 1.00
V = 78.351 L
Answer:
300000Pa or 3×10^5 Pa
Explanation:
Since the problem involves only two parameters of volume and pressure, the formula for Boyle's law is suitably used.
Using Boyle's law
P1V1 = P2V2
P1 is the initial pressure = 1.5×10^5Pa
V1 is the initial volume = 0.08m3
P2 is the final pressure (required)
V2 is the final volume = 0.04 m3
From the formula, P2 = P1V1/V2
P2 = 1.5×10^5 × 0.08 ÷ 0.04
= 300000Pa or 3×10^5 Pa.
Heat= mass * change in temperature* specific heat
specific heat=409 J/kg K
<h3><u>Answer;</u></h3>
C. 3Mg + Al2O3 → 3MgO + 2Al
<h3><u>Explanation;</u></h3>
- <u><em>Single replacement reaction is a type of reaction which one reactant reacts with another and makes a product by replacing one element by another. </em></u>
- Mg (Magnesium) reacts with Al₂O₃ (Aluminium oxide) and produces MgO (Magnesium oxide) and Al (Aluminium) as products. Here Al is replaced by Mg. Reaction is
Mg + Al₂O₃ → MgO + Al
- To balance the reaction equation, both left and right hand sides should have same number of atoms in each element.
The balanced equation will be;
3Mg + Al2O3 → 3MgO + 2Al
Explanation:
Considering the Henderson- Hasselbalch equation for the calculation of the pH of the buffer solution as:
pH=pKa+log[base]/[acid]
When the the concentrations of both buffer components (the weak acid and its conjugate base) are equal:
[base] = [acid]
So, pH=pKa+log1 = pKa
<u>pH is equal to pKa of weak acid of buffer system
.</u>
When buffer contains more of weak acid than conjugate base:
[base] < [acid]
log [base]/[acid] = Negative,
So,
<u>When more of acid component is present, the pH is more acidic. (It decreases)</u>
When buffer contains more of conjugate base than weak acid:
[base] > [acid]
log [base]/[acid] = Positive,
So,
<u>When more of acid component is present, the pH is more acidic. (It increases)</u>
