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belka [17]
3 years ago
15

A sample of atmospheric gas collected at an industrial site is stored in a 250 mL amber glass bottle that has a pressure of 1.02

atm and a temperature of 20.3°C. It was placed in an ice chest whose internal temperature is -2.0°C. What will be the new pressure of the gas sample once the gas temperature in the jar equilibrates to that of the ice chest?
Chemistry
2 answers:
UNO [17]3 years ago
8 0

I am looking for this answer too. Did you ever find it? I could really use the help

masha68 [24]3 years ago
3 0

Answer: The new pressure of the gas sample once the gas temperature in the jar 0.9424 atm.

Explanation:

Volume of the gas = 250 mL

Pressure of the gas at T_1=P_1

Pressure of the gas at T_2=P_2

At the constant volume pressure of the gas is directly proportional to the temperature of the gas in Kelvins that is Gay-Lussac's Law

P_1=1.02 atm , T_1=20.3^oC=293.3 K

P_2=? , T_2=-2^oC=271 K

\frac{P_1}{T_1}=\frac{P_2}{T_2}

\frac{P_1}{T_1}\times T_2=P_2=\frac{1.02 atm}{293.3 K}\times 271 K=0.9424 atm

The new pressure of the gas sample once the gas temperature in the jar 0.9424 atm.

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Calculate the percent of each component in the mixture. Show your calculations. Circle final answers.
Colt1911 [192]

Answer:

See Explanation

Explanation:

The question is incomplete; as the mixtures are not given.

However, I'll give a general explanation on how to go about it and I'll also give an example.

The percentage of a component in a mixture is calculated as:

\%C_E = \frac{E}{T} * 100\%

Where

E = Amount of element/component

T = Amount of all elements/components

Take for instance:

In (Ca(OH)_2)

The amount of all elements is: (i.e formula mass of (Ca(OH)_2))

T = 1 * Ca + 2 * H + 2 * O

T = 1 * 40 + 2 * 1 + 2 * 16

T = 74

The amount of calcium is: (i.e formula mass of calcium)

E = 1 * Ca

E = 1 * 40

E = 40

So, the percentage component of calcium is:

\%C_E = \frac{E}{T} * 100\%

\%C_E = \frac{40}{74} * 100\%

\%C_E = \frac{4000}{74}\%

\%C_E = 54.05\%

The amount of hydrogen is:

E = 2 * H

E = 2 * 1

E = 2

So, the percentage component of hydrogen is:

\%C_E = \frac{E}{T} * 100\%

\%C_E = \frac{2}{74} * 100\%

\%C_E = \frac{200}{74}\%

\%C_E = 2.70\%

Similarly, for oxygen:

The amount of oxygen is:

E = 2 * O

E = 2 * 16

E = 32

So, the percentage component of oxygen is:

\%C_E = \frac{E}{T} * 100\%

\%C_E = \frac{32}{74} * 100\%

\%C_E = \frac{3200}{74}\%

\%C_E = 43.24\%

5 0
3 years ago
How many grams (g) are in 0.250 moles of copper?
MissTica

Answer:

15.89grams

Explanation:

The mass of a substance can be calculated from it's mole value by using the formula:

mole = mass/molar mass

According to this question, there are 0.250 moles of copper. Hence, the mass of copper can be calculated as follows:

Molar mass of Cu = 63.55g/mol

0.250 = mass/63.55

mass = 0.250 × 63.55

mass = 15.8875

Mass of Cu in 0.250mol is 15.89grams.

5 0
3 years ago
If 448.85 mg of KOH is dissolved in 400 ml of water, what will be the pH of the solution?
emmasim [6.3K]
I have provided the steps and solution within the attachment. The pH of the solution would be 12.30, this indicates that the solution is basic, as a higher value of pH indicates presence of more hydroxide ions and less of hydrogen ions in the solution.

8 0
3 years ago
The following chemical equation is not balanced: Al + CuO Al2O3 + Cu When this chemical equation is correctly balanced, what is
Sergio039 [100]
2Al + 3CuO ----> Al2O3 + 3Cu

So the answer is 3
8 0
3 years ago
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How many grams of Fe are produced from 65.9 g of FeO given the following reaction: 3FeO + 2Al -> 3Fe +Al2O3
patriot [66]

Using the mole ratio and stoichiomrtery, you get:

65.9 g FeO x (molar mass of FeO) x (3 mol Fe/ 3 mol FeO) x (molar mass of Fe).

Plug in the values and you’re good to go!

8 0
3 years ago
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