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2 years ago

a gas exerts a pressure of 1.00 atm at 273 K. At what tempreture the gas exerts a pressure of 4.00 atm.

Chemistry

1 answer:

Diano4ka-milaya [45]2 years ago

8 0

Considering Gay-Lussac's law, a gas exerts a pressure of 4.00 atm at 1,092 K.

<h3>Gay-Lussac's law</h3>

Gay-Lussac's law states that the pressure of a gas is directly proportional to its temperature: when there is a constant volume, as the temperature increases, the pressure of the gas increases. And when the temperature is decreased, gas pressure decreases.

Gay-Lussac's law can be expressed mathematically as follows:

$\frac{P}{T}=k$

where P= pressure, T= temperature, k= Constant

This law states that the ratio of pressure to temperature is constant.

Studying an initial state 1 and a final state 2, it is fulfilled:

$\frac{P1}{T1}=\frac{P2}{T2}$

<h3>Final temperature</h3>

In this case, you know:

P1= 1 atm
T1= 273 K
P2= 4 atm
T2= ?

Replacing in Gay-Lussac's law:

$\frac{1 atm}{273 K}=\frac{4 atm}{T2}$

Solving:

$T2\frac{1 atm}{273 K}=4 atm$

$T2=\frac{4 atm}{\frac{1 atm}{273 K}}$

Finally, a gas exerts a pressure of 4.00 atm at 1,092 K.

Learn more about Gay-Lussac's law:

brainly.com/question/4147359

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A 7.0 g sample of a hydrocarbon (a molecule that has only hydrogen and carbon) is subject to combustion analysis. The mass of CO

Akimi4 [234]

Answer: The empirical formula for the given compound is $CH_2$

Explanation:

The chemical equation for the combustion of compound having carbon and hydrogen follows:

$C_xH_y+O_2\rightarrow CO_2+H_2O$

where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.

We are given:

Mass of $CO_2=22.0g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 22.0 g of carbon dioxide, $\frac{12}{44}\times 22.0=6g$ of carbon will be contained.

For calculating the mass of hydrogen:

Mass of hydrogen = Mass of sample - Mass of carbon

Mass of hydrogen = 7.0 g - 6 g

Mass of hydrogen = 1.0 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{6g}{12g/mole}=0.5moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1.0g}{1g/mole}=1.0moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.5 moles.

For Carbon = $\frac{0.5}{0.5}=1$

For Hydrogen = $\frac{1.0}{0.5}=2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of Fe : C : H = 1 : 2

Hence, the empirical formula for the given compound is $C_{1}H_{2}=CH_2$

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3 years ago

How do you do this? very confused

Vlad [161]

The problem you have written you almost have it solved. Take the moles that you have calculated and multiply that by the molecular weight to get the grams.

The STP problem:
use the moles you calculated along with 1 atm for Pressure, and 273 for the temperature and plug into the PV = nRT equation. (also use 0.0821 for R)

From there you can solve for the volume

Hope this helps!

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Palmitic acid C16H32O2 is a dietary fat found in beef and butter. The caloric content of palmitic acid is typical of fats in gen

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C16H32O2(aq) --> 16CO2(g) + 16H2O(l) ... said its wrong though?
<span>This is because you haven't added any oxygen needed for the combustion, so your equation does'nt balance. Also a solution in water [aq] doesn't burn! </span>
<span>Try </span><span>C16H32O2(s) + 23O2(g) --> 16CO2(g) + 16H2O(l)

Thank you for posting your question here at brainly. I hope the answer will help you. Feel free to ask more questions.
</span>

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