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lesantik [10]
3 years ago
14

Determine which law is appropriate for solving the following problem. Carbon dioxide is in a steel tank at 20°C, 10 liters and 1

atm. What is the pressure on the gas when the tank is heated to 100°C? Law used:
Chemistry
2 answers:
patriot [66]3 years ago
5 0

<u>Answer:</u>

Law used: Combined Gas Law

<u>Explanation:</u>

We are given the following problem:

Carbon dioxide is in a steel tank at 20°C, 10 liters and 1 atm. What is the pressure on the gas when the tank is heated to 100°C?

To solve this, the most appropriate law that can be used it Combined Gas Law, which is the result of combining the Boyle's law, Charles' law, and Gay-Lussac's law together.

Alex17521 [72]3 years ago
3 0

Answer : The final pressure will be, 1.27 atm

Explanation :

Gay-Lussac's Law : It is defined as the pressure of the gas is directly proportional to the temperature of the gas at constant volume and number of moles.

P\propto T

or,

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

where,

P_1 = initial pressure of gas = 1 atm

P_2 = final pressure of gas = ?

T_1 = initial temperature of gas = 20^oC=273+20=293K

T_2 = final temperature of gas = 100^oC=273+100=373K

Now put all the given values in the above equation, we get:

\frac{1atm}{293K}=\frac{P_2}{373K}

P_2=1.27atm

Thus, the final pressure will be, 1.27 atm

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3 years ago
Calculate the theoretical yield of ammonia produced by the reaction of 100g of H2 gas and 200g of N2 gas
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To get the theoretical yield of ammonia NH3:
first, we should have the balanced equation of the reaction:
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moles of N2 = N2 mass / N2 molar mass
                     = 200 / 28 = 7.14 moles
third, we start to compare the molar ratio from the balanced equation between N2 & NH3 we will find that N2: NH3 = 1:2 so when we use every mole of N2 we will get 2 times of that mole of NH3 so,
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3 years ago
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6 0
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Problem PageQuestion Methane gas and chlorine gas react to form hydrogen chloride gas and carbon tetrachloride gas. What volume
IgorC [24]

Methane gas and chlorine gas react to form hydrogen chloride gas and carbon tetrachloride gas. What volume of hydrogen chloride would be produced by this reaction if 3.16 L of chlorine were consumed at STP.

Be sure your answer has the correct number of significant digits.

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Explanation:

According to ideal gas equation:

PV=nRT

P = pressure of gas = 1 atm  (at STP)

V = Volume of gas = 3.16 L

n = number of moles = ?

R = gas constant =0.0821Latm/Kmol

T =temperature =273K=

n=\frac{PV}{RT}

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Thus volume of carbon tetrachloride that would be produced is 0.788 L

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