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Lapatulllka [165]
3 years ago
5

if the caffeine concentration in a particular brand of soda is 2.87 mg/oz, drinking how many cans of soda would be lethal? assum

e 10.0 grams of caffeine is a lethal dose, and there are 12 oz in a can.
Chemistry
1 answer:
aleksklad [387]3 years ago
4 0
Approximately 290 drinks would be lethal
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A student used 1.2 g of hydrate in the first trial and 1.6 g in the second trial. Explain fully why her mass percent of water wi
Pachacha [2.7K]

Both trials of 1.2 g and 1.6 g will have the same mass percent of water because the ratio of the salt to the water of hydration is always constant for any hydrated salt.

<h3>Water of hydration</h3>

For every hydrated salt, the ratio of the salt to the water of hydration remains constant irrespective of the amount of salt taken for experimental analysis.

For example, assuming the mass percent of water in 10g of a hydrated salt is 40%, if 100g of the same salt is taken, the mass percent will remain 40%.

More on water of hydration can be found here: brainly.com/question/11202174

8 0
2 years ago
What does ethylene glycol do to the solution in a vehicle’s radiator? It raises the boiling point and lowers the freezing point.
zheka24 [161]

Answer:

It raises the boiling point and lowers the freezing point.

Explanation:

It is used as antifreeze in the cooling circuits of internal combustion engines, that is, it is used to reduce the melting point of the solution.

By adding ethylene glycol I'm not only bringing the melting point to -13°C, but the boiling point of ethylene glycol is 197°C.

since these substances not only lower the freezing point but also increase the boiling point, they are also called a colligative agent

5 0
3 years ago
Read 2 more answers
What is the vapor pressure of a solution in which the mole fraction of the solute is 0.200 and the vapor pressure of the pure so
Ulleksa [173]

Answer: The vapor pressure of a solution in which the mole fraction of the solute is 0.200 is 80.0 torr

Explanation:

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

\frac{p^o-p_s}{p^o}=i\times x_2

where,

p^0= vapor pressure of pure solvent = 100.0 torr

p_s = vapor pressure of solution = ?

i = Van'T Hoff factor = 1 for nonvolatile, nonelectrolyte solute

x_2 = mole fraction of solute  = 0.200  

\frac{100.0-p_s}{100.0}=1\times 0.200

p_s=80.0torr

The vapor pressure of a solution in which the mole fraction of the solute is 0.200 is 80.0 torr

7 0
3 years ago
Convert 2.25 millimol to mole.
77julia77 [94]

the conversion would be 0.00225 mole

6 0
3 years ago
The substance fluorine has the following properties: normal melting point: 53.5 K normal boiling point: 85.0 K triple point: 1.6
mihalych1998 [28]

Answer:

The true statements include;

- The sample is initially a gas.

- The final state of the substance is a solid.

- One or more phase changes will occur.

The untrue/false statements include;

- The liquid initially present will vaporize.

- The final state of the substance is a liquid.

Explanation:

A couple pieces of informatton on Fluorine is imitially provided.

The substance fluorine has the following properties: normal melting point: 53.5 K normal boiling point: 85.0 K triple point: 1.6×10-4 atm, 53.4 K critical point: 55 atm, 144.1 K

So, a question is now attached about a sample of Fluorine. A sample of fluorine at a pressure of 1.00 atm and a temperature of 90.3 K is cooled at constant pressure to a temperature of 49.3 K.

We are then told to examine a group of options to find the ones that are correct/apply.

Taking the options one at a time

- The sample is initially a gas.

The initial state of the Fluorine sample has its temperature at 90.3 K, which is above the gas' boiling point. Hence, the sample can be concluded to initially be a gas.

- The liquid initially present will vaporize.

The sample doesn't initially contain liquid. And even of it did, the temperature is cooled, not heated , Hence, this statement is wrong.

- The final state of the substance is a solid.

The sample of Fluorine moves from a temperature higher than boiling point (85.0 K), with the sample in gaseous form, to one that is at a lower temperature (49.3 K) than the gas' normal melting point (53.5 K).

At temperatures lower than melting point, a substance exists in the solid form. Hence, this statement is true. The final state of the substance is solid.

- One or more phase changes will occur.

In moving from 90.3 K to 49.3 K for the sample and passing through the substance's boiling and melting points (85.0 K and 53.5 K respectively) along the way, it is logical to conclude that there would be one or more phase changes will occur. This statement is true.

- The final state of the substance is a liquid.

This is false as we already established that the final state of the substance is a solid. Hence, this statement is false.

Hope this Helps!!!

7 0
3 years ago
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