Answer:
Multiply 1.25 by 0.04 and divide the result obtained by 1,000
Explanation:
Given: [1 gram = 0.04 ounce, 1 liter = 1,000 milliliter]
1.25 x 0.04 = 0.05 oz
Therefore, 0.05 per 1,000 milliliter
0.05 ÷ 1,000 = 0.00005 oz
Therefore, the density of the gas is 0.00005 oz/mL
Hope this helps! :)
Answer:
% = 76.75%
Explanation:
To solve this problem, we just need to use the expressions of half life and it's relation with the concentration or mass of a compound. That expression is the following:
A = A₀ e^(-kt) (1)
Where:
A and A₀: concentrations or mass of the compounds, (final and initial)
k: constant decay of the compound
t: given time
Now to get the value of k, we should use the following expression:
k = ln2 / t₁/₂ (2)
You should note that this expression is valid when the reaction is of order 1 or first order. In this kind of exercises, we can assume it's a first order because we are not using the isotope for a reaction.
Now, let's calculate k:
k = ln2 / 956.3
k = 7.25x10⁻⁴ d⁻¹
With this value, we just replace it in (1) to get the final mass of the isotope. The given time is 1 year or 365 days so:
A = 250 e^(-7.25x10⁻⁴ * 365)
A = 250 e^(-0.7675)
A = 191.87 g
However, the question is the percentage left after 1 year so:
% = (191.87 / 250) * 100
<h2>
% = 76.75%</h2><h2>
And this is the % of isotope after 1 year</h2>
Supposing complete ionization:
<span>CaCl2 → Ca{2+} + 2 Cl{-} [three ions total] </span>
<span>(1.56 m CaCl2) x (3 mol ions / 1 mol CaCl2) = 4.68 m ions </span>
<span>(1.86 °C/m) x (4.68 m) = 8.70 °C change </span>
<span>0°C - 8.70°C = - 8.70°C</span>
The pressure has almost no effect on the solubilities of solids and liquids. If a solid is insoluble in a liquid we cannot increase its solubility in that liquid by applying pressure. Similarly if two liquids are immiscible, we cannot dissolve them in each other by applying pressure. If two liquids are miscible, even if you don't apply any pressure they mix in every proportion.
<span>However, the solubilities of gases in liquids are directly proportional to the pressure applied to the gases. Remember the fizzy drinks in which CO2 gas is dissolved under very high pressure. As far as the bottle is opened, pressure decreases and most of the dissolved gas try to escape from the liquid. </span>
