Use the state equation for ideal gases: pV = nRT
Data:
V = 88.89 liter
n = 17 mol
T = 67 + 273.15 = 340.15 K
R = 0.0821 atm * liter / (K*mol)
=> p = nRT / V = 17 mol * 0.0821 (atm*liter / K*mol) * 340.15 K / 88.89 liter
p = 5.34 atm
Answer: p = 5.34 atm
6_____18 record your data to be used in the following problem.
Answer: The boiling points of the two liquids are quickly exceeded
Explanation:
Fractional distillation is a method of separating a mixture of liquids where each has different boiling points.
To therefore obtain individual fractions, temperature rise of the mixture must be gradual, otherwise the boiling points of the two liquids will be quickly exceeded making collection of each fraction impossible.
Answer:
1.5 moles of H₂SO₄ needs 3.0 moles pf KOH to be neutralized.
Explanation:
- KOH is dissociate according to the equation:
KOH → K⁺ + OH⁻.
- H₂SO₄ is dissociated according to the equation:
H₂SO₄ → 2H⁺ + SO₄²⁻.
<em>So, every 1.0 mole of KOH produces 1.0 mol of OH⁻.</em>
<em>While, every 1.0 mole of H₂SO₄ produces 1.0 mol of H⁺.</em>
<em />
Thus, every mol of H₂SO₄ needs 2.0 moles of KOH to be neutralized.
<em>So, 1.5 moles of H₂SO₄ needs (2 x 1.5 mol) = 3.0 moles pf KOH to be neutralized.</em>
<span>Yes, mass is conserved.
In any chemical reaction mass is neither created, nor destroyed. That is a basic principle that remained unaltered and unchallenged until the discovery of nuclear power. And even then, the basic principle of conservation of mass was simply altered to include the conservation of energy as well. If you with to demonstrate this conservation by the reaction of sodium hydroxide with copper sulfate, you can do so by measuring the mass of all reactants and reaction vessels both before and after the reaction. Just put the beaker with sodium hydroxide solution along with the beaker of copper sulfate solution on the balance scale and measure their total mass. Then pour one solution into the other, and place both the full beaker with the reactants and product as well as the empty beaker back on the balance scale and measure their combined mass. If you perform the measurements accurately, the combined masses both before and after the reaction will be identical.</span>
