you are right on all the ones you did
Answer:
Option D is correct.
Explanation:
Compared to a sample of helium at STP, the same sample of helium at a higher temperature and a lower pressure because any gas at a higher temperature and a lower pressure will behaves like an ideal gas. for eg.
nitrogen at STP show its behavior as an ideal gas.
When pressure of a gas increased & temperature is decreased then the gas does not follow ideal gas law.
Therefore option D is correct.
Answer:
The answer to your question is: 6 ml of HCl
Explanation:
1.- Molarity of NaCl in solution
n = # of moles
M = n / volume (l)
n = M x v
n = (0.1) (0.030)
n = 0.003 moles of NaOH
2.- Number of moles of HCl that react
From the reaction 1 mol of NaOH ----------------- 1 mol of HCl
0.003 moles ----------------- x
x = (0.003 x 1) / 1 = 0.003 moles of HCl
3.- Volume of HCl that react
M = n/ V
V = n / M
V = 0.003 / 0.5
V = 0.006 l
V = 6 ml
Answer:
Na⁺ (aq) + OH⁺ (aq) + H⁺ (aq) + Cl⁻ (aq) → Na⁺ (aq) + Cl⁻ (aq) + H₂O (l)
General Formulas and Concepts:
<u>Atomic Structure</u>
<u>Aqueous Solutions</u>
- Solubility Rules
- States of matter
<u>Stoichiometry</u>
- Reaction RxN Prediction
- Balancing Reactions RxN
Explanation:
<u>Step 1: Define</u>
NaOH reacting w/ HCl
NaOH is soluble
HCl is soluble
[RxN] NaOH (aq) + HCl (aq) → NaCl (aq) + H₂O (l)
<u>Step 2: Total Ionic Equation</u>
<em>Break up soluble compounds into ionic form.</em>
[T.I.E] Na⁺ (aq) + OH⁺ (aq) + H⁺ (aq) + Cl⁻ (aq) → Na⁺ (aq) + Cl⁻ (aq) + H₂O (l)
False<span>: </span>Liquid<span> and solid water are in equilibrium at this</span>temperature<span> and </span>pressure, so ∆G<span>=0.</span>
