Answer:
The partial pressure of SO₃ is measured at 82.0 atm.
Explanation:
The equilibrium constant Kp is defined as the ratio of the equilibrium pressures of the gaseous products, each raised to the power of their respective coefficients in the reaction, divided by the pressures of the gaseous reactants raised to their coefficients.
For the given reaction,
2 SO₂(g) + O₂(g) → 2 SO₃(g)
![Kp = 0.345 = \frac{(pSO_{3})^{2} }{(pSO_{2})^{2} \times pO_{2} }\\pSO_{3} = \sqrt[]{0.345 \times (pSO_{2})^{2} \times pO_{2} } \\pSO_{3} = \sqrt[]{0.345 \times (35.0)^{2} \times 15.9 } \\pSO_{3} = 82.0 atm](https://tex.z-dn.net/?f=Kp%20%3D%200.345%20%3D%20%5Cfrac%7B%28pSO_%7B3%7D%29%5E%7B2%7D%20%7D%7B%28pSO_%7B2%7D%29%5E%7B2%7D%20%5Ctimes%20pO_%7B2%7D%20%7D%5C%5CpSO_%7B3%7D%20%3D%20%5Csqrt%5B%5D%7B0.345%20%5Ctimes%20%28pSO_%7B2%7D%29%5E%7B2%7D%20%5Ctimes%20pO_%7B2%7D%20%7D%20%5C%5CpSO_%7B3%7D%20%3D%20%5Csqrt%5B%5D%7B0.345%20%5Ctimes%20%2835.0%29%5E%7B2%7D%20%5Ctimes%2015.9%20%7D%20%5C%5CpSO_%7B3%7D%20%3D%2082.0%20atm)
Answer:
H+(aq) + OH-(aq) ⟶ H2O(l)
Explanation:
Step 1: The balanced equation can be presented as
HCN(aq) + KOH(aq) ⟶ H2O(l) + KCN(aq)
H+(aq) + CN-(aq) + K+(aq) + OH-(aq) ⟶ H2O(l) + K+(aq) + CN-(aq)
Step 2: The net ionic equation is formed by removing the spectator ions — those that appear on both sides of the equation — leading us to the final representation:
H+(aq) + OH-(aq) ⟶ H2O(l)
<span>Some solutions demonstrate colligative properties, which rely on the quantity of solute in a solvent. To find the elevation in boiling point, we use the formula:
</span><span>ΔT(boiling point) =
(Kb)mi
where Kb represents a constant, m is the solution's molality, and i is the van't Hoff factor.
From the provided information, we can easily determine i as follows:
</span>ΔT(boiling point) = (Kb)mi
103.45 - 100 = (0.512)3.90i
i = 1.73 <-------van't Hoff factor
Answer:
Explanation:
Given data:
Initial temperature T₁ = 25.2°C = 298.2K
Initial pressure P₁ = 0.6atm
Final temperature = 72.4°C = 345.4K
What we need to find:
Final pressure = ?
To determine this, we apply a modified version of the combined gas law with constant volume. This simplifies our calculations to:
Here, P and T signify pressure and temperatures, 1 refers to initial and 2 to final temperatures.
Now we can substitute the known variables:
P₂ = 0.7atm
Answer:
- A. Which element, X or Z, has a higher molar mass?
Explanation:
Heating the original compounds intensely to remove all oxygen causes chemical decomposition reactions:
- 2XClO₃ (solid) → 2XCl + 3O₂ (gas)
- 2ZClO₃ (solid) → 2ZCl + 3O₂ (gas)
By measuring the initial mass of each sample and the mass remaining after heating, the student can compute the oxygen gas mass released:
- Mass of oxygen released = initial sample mass minus residue mass
Using this oxygen mass, she can calculate how many moles of oxygen were present in each sample:
- Moles of oxygen = oxygen mass (g) divided by molar mass of oxygen
Next, the moles of the original sample are determined:
- Each mole of XClO₃ or ZClO₃ has 3 moles of oxygen atoms.
So, dividing the moles of oxygen released by 3 gives the moles of the sample.
Applying the formula molar mass = mass / moles, the student finds the molar masses of XClO₃ and ZClO₃.
Thus, this data allows answering question A: Which of X or Z has the higher molar mass?
