Answer:
Carbon dioxide (CO₂)
Explanation:
Carbonic acid decomposes to release water and carbon dioxide:
H₂CO₃ → H₂O + CO₂
In an aqueous solution, it has this two equilibriums where it release 2 protons. It is a weak acid:
H₂CO₃ + H₂O ⇄ HCO₃⁻ + H₃O⁺ Ka₁
HCO₃⁻ + H₂O ⇄ CO₃⁻² + H₃O⁺ Ka₂
Answer:
90.4 mL
Explanation:
Step 1: Given data
- Initial volume of the gas (V₁): 113 mL
- Initial pressure of the gas (P₁): 721 mmHg
- Final volume of the gas (V₂): ?
- Final pressure of the gas (P₂): 901 mmHg
Step 2: Calculate the final volume of the gas
According to Boyle's law, the volume of a gas is inversely proportional to the pressure. We can calculate the final volume of the gas using the following expression.
P₁ × V₁ = P₂ × V₂
V₂ = P₁ × V₁ / P₂
V₂ = 721 mmHg × 113 mL / 901 mmHg
V₂ = 90.4 mL
Answer:
25 mL
Explanation:
The reaction that takes place is:
- Ca(OH)₂ + 2HNO₃ → Ca(NO₃)₂ + 2H₂O
First we<u> calculate how many Ca(OH)₂ moles</u> were spent in the titration:
- 25.0 mL * 0.100 M = 2.5 mmol Ca(OH)₂
Then we <u>convert Ca(OH)₂ moles into HNO₃ moles</u>, using the <em>stoichiometric ratio</em>:
- 2.5 mmol Ca(OH)₂ *
= 5.0 mmol HNO₃
Finally we <u>calculate the volume of required nitric acid solution</u>, using the <em>concentration</em>:
- 5.0 mmol ÷ 0.200 mmol/mL = 25 mL
Answer:
The volume is 59, 3 liters. See the explanation below, please
Explanation:
STP conditions (standard) correspond to 273K of temperature and 1 atm of pressure. These values are used and the volume is calculated, according to the formula:
PV = nRT
1 atm x V= 2, 65 moles x 0, 082 l atm/K mol x 272 K
V= 2, 65 moles x 0, 082 l atm/K mol x 272 K/1 atm = 59, 3 liters
