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12 days ago

Vinegar is an aqueous solution of acetic acid, ch3cooh. a 5.00 ml sample of a particular vinegar requires 26.90 ml of 0.175 m na

oh for its titration. what is the molarity of acetic acid in the vinegar?

Chemistry

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1. If a car is traveling 90 mi/hr, how many feet will the car travel in 1 sec? In 5 sec?

alisha [2963]

Answer:

The vehicle travels 660 feet

Explanation:

Initially, convert the speed into Feet per second

The car's speed is 90 mi/hr

1 mi = 5280 ft

For 90 miles, we calculate 90 x 5280 = 475,200 feet

1 hour = 60 minutes

1 minute = 60 seconds

Therefore,

1 hour = 60 x 60 seconds = 3600 seconds

Speed is defined as the distance covered by an object over time. The speed formula is:

$Speed =\frac{distance}{time}$

$Speed =\frac{90mi}{1hr}$ ... given

$Speed =\frac{475200 ft}{3600sec}$

Speed = 132 ft/sec

Thus, time = 5 seconds

$Speed =\frac{distance}{time}$

$distance =speed\times time$

$distance = 132ft/sec\times 5sec$

Distance = 660 feet

3 0

3 months ago

Combustion analysis of a 13.42-g sample of the unknown organic compound (which contains only carbon, hydrogen, and oxygen) produ

lions [2927]

Answer: The molecular formula for the specified organic compound is $C_{18}H_{20}O_2$

Explanation:

The combustion reaction of a hydrocarbon comprising carbon, hydrogen, and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where 'x', 'y', and 'z' denote the subscripts of Carbon, hydrogen, and oxygen respectively.

The information provided includes:

Mass of $CO_2=39.61g$

Mass of $H_2O=9.01g$

From our knowledge:

Molar mass of carbon dioxide is 44 g/mol

Molar mass of water is 18 g/mol

For determining the amount of carbon:

In carbon dioxide weighing 44 g, 12 g of carbon is found.

Hence, in 39.61 g of carbon dioxide, $\frac{12}{44}\times 39.61=10.80g$ grams of carbon will be found.

For finding the mass of hydrogen:

In water weighing 18 g, 2 g of hydrogen can be found.

Thus, in 9.01 g of water, $\frac{2}{18}\times 9.01=1.00g$ grams of hydrogen will be present.

Mass of oxygen in the compound is given by (13.42) - (10.80 + 1.00) = 1.62 g

To derive the empirical formula, the following steps must be followed:

Step 1: Convert the indicated masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{10.80g}{12g/mole}=0.9moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1g}{1g/mole}=1moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{1.62g}{16g/mole}=0.10moles$

Step 2: Calculating the ratio of moles of the respective elements.

To find the mole ratio, each mole value is divided by the smallest amount of moles calculated, which is 0.10 moles.

For Carbon = $\frac{0.9}{0.10}=9$

For Hydrogen = $\frac{1}{0.10}=10$

For Oxygen = $\frac{0.10}{0.10}=1$

Step 3:Using the mole ratios as subscripts.

The ratio of C: H: O = 9: 10: 1

Therefore, the empirical formula for the mentioned compound is $C_9H_{10}O$

To ascertain the molecular formula, it is necessary to find the valency, which is multiplied by each element to derive the molecular formula.

The equation to determine the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

Given the data:

Molecular formula mass = 268.34 g/mol

Empirical formula mass = 134 g/mol

Substituting the values into the aforementioned equation yields:

$n=\frac{268.34g/mol}{134g/mol}=2$

By multiplying this valency with each element's subscripts from the empirical formula, the results are:

$C_{(9\times 2)}H_{(10\times 2)}O_{(1\times 2)}=C_{18}H_{20}O_2$

Consequently, the molecular formula for the given organic compound is $C_{18}H_{20}O_2$ .

3 0

2 months ago

While hiking in the woods, you see a brown, rotting apple lying on the ground. What changes is the physical properties of the ap

eduard [2782]

Response:

The alteration in color.

Explanation:

The apple browns due to the oxidation process. This occurs when oxygen and water molecules from the air interact with it, resulting in oxidation. The oxidation process is notably rapid at room temperature.

For instance, if the peeled apple is placed in the refrigerator, it takes longer to oxidize and turn brown, but if left at room temperature, it quickly turns brown.

When oxygen interacts with the peeled apple, it activates the polyphenol oxidase enzyme, oxidizing the phenolic compounds and forming quinones, which then react with amino acids to create the brown coloration.

3 0

2 months ago