Answer:
1) 2.054 x 10⁻⁴ mol/L.
2) Decreasing the temperature will increase the solubilty of O₂ gas in water.
Explanation:
1) The solubility of O₂ gas in water:
- We cam calculate the solubility of O₂ in water using Henry's law: <em>Cgas = K P</em>,
- where, Cgas is the solubility if gas,
- K is henry's law constant (K for O₂ at 25 ̊C is 1.3 x 10⁻³ mol/l atm),
- P is the partial pressure of O₂ (P = 120 torr / 760 = 0.158 atm).
- Cgas = K P = (1.3 x 10⁻³ mol/l atm) (0.158 atm) = 2.054 x 10⁻⁴ mol/L.
2) The effect of decreasing temperature on the solubility O₂ gas in water:
- Decreasing the temperature will increase the solubilty of O₂ gas in water.
- When the temperature increases, the solubility of O₂ gas in water will decrease because the increase in T will increase the kinetic energy of gas particles and increase its motion that will break intermolecular bonds and escape from solution.
- Decreasing the temperature will increase the solubility of O₂ gas in water will because the kinetic energy of gas particles will decrease and limit its motion that can not break the intermolecular bonds and increase the solubility of O₂ gas.
Answer:
100 HZ 1,000 HZ 10,000 HZ there you go :)
The final temperature on increasing the pressure to 7.65 atm is 637 K.
Explanation:
The relation between temperature attained by gas molecules at varying pressure is defined by Guy-Lusac's law. It states that at constant volume, the pressure experienced by the gas molecules is directly proportional to the temperature attained by those molecules.
P∝T
Here, the initial pressure P₁ is given as 4 atm at temperature T₁ = 333 K, then the final pressure P₂ = 7.65 atm can be attained at temperature T₂.
The final temperature should be greater than the initial temperature as there is an increase in the pressure.
So,
Hence, the final temperature on increasing the pressure to 7.65 atm is 637 K.
Answer:
Explanation:
Hello!
In this case, since the formula for the calculation of molarity is defined in terms of moles and volume in liters as shown below:
Whereas the moles are computed by considering the molar mass of CaCO3 (100.09 g/mol):
Thus, we obtain:
Best regards!
From the Avogadro's law one mole of a substance contains 6.022× 10^23 particles.
Therefore; 1 mole of water contains 6.022 × 10^23 molecules
Hence 1.7 moles will contain;
1.7 × 6.022 × 10^23 molecules
= 10.2374 × 10^23 molecules
= 1.024 ×10^24 molecules
≈ 1.02 × 10^24 molecules