Answer:
<h2>Density = 12.5 g/mL</h2>
Explanation:
The density of a substance can be found by using the formula
From the question
mass = 52.5 g
volume = 4.2 mL
Substitute the values into the above formula and solve for the density
We have
We have the final answer as
<h3>Density = 12.5 g/mL</h3>
Hope this helps you
Answer:
3) 2KOH + H2SO4 → K2SO4 + 2H2O
Explanation:
The balanced chemical equation for the reaction of KOH and H2SO4 is,
→ 2KOH + H2SO4 → K2SO4 + 2H2O
Hence, option (3) is the correct answer.
Answer:
127°C
Explanation:
This excersise can be solved, with the Charles Gay Lussac law, where the pressure of the gas is modified according to absolute T°.
We convert our value to K → -73°C + 273 = 200 K
The moles are the same, and the volume is also the same:
P₁ / T₁ = P₂ / T₂
But the pressure is doubled so: P₁ / T₁ = 2P₁ / T₂
P₁ / 200K = 2P₁ / T₂
1 /2OOK = (2P₁ / T₂) / P₁
See how's P₁ term is cancelled.
200K⁻¹ = 2/ T₂
T₂ = 2 / 200K⁻¹ → 400K
We convert the T° to C → 400 K - 273 = 127°C
Answer:
41.1%
Explanation:
First write the balanced reaction:
CaCO₃ + H₂SO₄ → CaSO₄ + H₂O + CO₂
Now calculate the theoretical yield:
49.3 g CaCO₃ × (1 mol CaCO₃ / 100 g CaCO₃) = 0.493 mol CaCO₃
0.493 mol CaCO₃ × (1 mol H₂O / 1 mol CaCO₃) = 0.493 mol H₂O
0.493 mol H₂O × (18 g H₂O / mol H₂O) = 8.87 g H₂O
Now calculate the % yield:
3.65 g H₂O / 8.87 g H₂O × 100% = 41.1%
