They tell you to have caution.
It is a physical change because it is still the same thing (a pretzel) but just in two pieces. You’re not changing chemical composition.
Answer:
a. n = 6,54 moles.
b. CH₃COOH(aq) + NaHCO₃(aq) → CH₃COONa(aq) + H₂O (l) + CO₂(g)
c. 549g of NaHCO₃
d. 7,85L of CH₃COOH
Explanation:
a. It is possible to know moles of CO₂ required to inflate the air bag using:
n = PV/RT
Where n are moles; P is pressure (1atm at room conditions); V is volume (160L); R is gas constant (0,082 atmL/molK); and T is temperature (298,15K at room conditions.
Replacing:
<em>n = 6,54 moles.</em>
b. The reaction of CH₃COOH with NaHCO₃ produce:
CH₃COOH(aq) + NaHCO₃(aq) → CH₃COONa(aq) + H₂O (l) + CO₂(g)
c. 1 mol of CO₂ is produced from 1 mol of NaHCO₃, that means 6,54moles of CO₂ are produced from <em>6,54 moles of NaHCO₃</em>. In grams:
6,54 moles NaHCO₃×
= <em>549g of NaHCO₃</em>
d. Again, you require 6,54 moles of CH₃COOH. If your acetic acid solution is 0,833M you need:
6,54moles×
= <em>7,85L of CH₃COOH</em>
<em></em>
I hope it helps!
Answer:
its a chemical formula, it has numbers and symbols
Answer:
a) At a given temperature, C₂H₆ has a higher vapor pressure than C₄H₁₀.
Explanation:
<em>Which statement below is true?
</em>
<em>a) At a given temperature, C₂H₆ has a higher vapor pressure than C₄H₁₀. </em>TRUE. C₂H₆ has a lower molar mass than C₄H₁₀ and a higher vapor pressure at most temperatures.
<em>b) The strongest intermolecular attractive forces present in liquid CCl₄ are dipole-dipole forces.</em> FALSE. CCl₄ is nonpolar, so the strongest intermolecular forces are dispersion forces.
<em>c) HCl has a higher boiling point than LiCl.</em> FALSE. LiCl (ionic compound) has a higher boiling point than HCl (covalent compound).
<em>d) H₂O has a greater polarizability than H₂Se.</em> FALSE. Se has a larger atomic radius than O which is why H₂Se has a greater polarizability than H₂O.
<em>e) In general, the stronger the intermolecular attractive forces, the lower the ∆Hºvap.</em> FALSE. In general, the stronger the intermolecular attractive forces, the higher the ∆Hºvap.
