Answer:
437.5 kg of first solution and 812.5 kg of second solution should be mixed to get desired solution.
Explanation:
Let the mass of the first solution be x and second solution be y.
Amount solution required = 1250 kg
x + y = 1250 kg....[1]
Percentage of ethanol in required solution = 12% of 1250 kg
Percentage of ethanol in solution-1 = 5% of x
Percentage of ethanol in required solution = 25% of y
5% of x + 25% of y =12% of 1250 kg

x + 5y = 3000 kg...[2]
Solving [1] and [2] we :
x = 437.5 kg , y = 812.5 kg
437.5 kg of first solution and 812.5 kg of second solution should be mixed to get desired solution.
$6.72/lb = $6.72/16 oz = $0.42/oz = 42 cents per ounce
<span>RE: "numerically to the hundredths place." </span>
<span>Since, in this case, you're dealing with money, "the hundredths place" simply means, "to the nearest cent."</span>
Explanation:
When we are using spoon, beaker, stirring rod and graduated cylinder then they directly come in contact with the chemical we are using. Hence, if they are not washed thoroughly then chemicals remain deposited over them.
As a result, when successive test are performed using the same contaminated apparatuses then we do not get the desired results.
Whereas distilled water in a spray bottle if poured without touching or coming in contact with any kind of chemicals.
Hence, we can conclude that spoon, beaker, stirring rod and graduated cylinder are the tools that could have become cross-contaminated during the experiment if you had not cleaned them carefully between successive tests.
Answer:
a. Yes
b. 143.5 mmHg
Explanation:
The vapor pressure is the pressure of the vapor that is in equilibrium with the liquid. At a constant temperature, some molecules of the liquid will vaporize, and then will do pressure at the surface of the liquid.
If the pressure at the container is higher then the vapor pressure, the liquid will evaporate.
a. Let's calculate the pressure at the container by the ideal gas law:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (62,364 mmHg.mL/mol.K), and T is the temperature.
The molar mass of CH₃I is 142 g/mol
n = mass/ molar mass
n = 0.453/142
n = 0.0032 mol
P*370 = 0.0032*62,364*266
370P = 53,084.24
P = 143.5 mmHg
So, all the liquid will evaporate.
b. Because all liquid evaporates, when the equilibrium is reached, the pressure is the gas pressure: 143.5 mmHg.
We can use a simple equation to solve this problem.
d = m/v
Where d is the density, m is the mass and v is the volume.
d = ?
m = 87.47 mg = 87.47 x 10⁻³ g
v = 0.03 mL
By applying the equation,
d = 87.47 x 10⁻³ g
/ 0.03 mL
d = 2.92 g/mL
Hence, the density of the mixture is 2.92 g/mL.