CHEMISTRY MIDDLE SCHOOL

If I initially have a gas at a pressure of 12 atm, volume of 23 liters, and temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?

Answers

Answer 1

Answer:

Answer : The volume of gas will be 29.6 L

Explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

$(P_1V_1)/(T_1)=(P_2V_2)/(T_2)$

where,

$P_1$ = initial pressure of gas = 12 atm

$P_2$ = final pressure of gas = 14 atm

$V_1$ = initial volume of gas = 23 L

$V_2$ = final volume of gas = ?

$T_1$ = initial temperature of gas = 200K

$T_2$ = final temperature of gas = 300K

Now put all the given values in the above equation, we get the final pressure of gas.

$(12atm* 23L)/(200K)=(14* V_2)/(300K)$

$V_2=29.6L$

Therefore, the new volume of gas will be 29.6 L

Answer 2

Answer:

Hello!

If I initially have a gas at a pressure of 12 atm, volume of 23 liters, and temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?

We have the following data:

P1 (initial pressure) = 12 atm

V1 (initial volume) = 23 L

T1 (initial temperature) = 200 K

P2 (final pressure) = 14 atm

T2 (final temperature) = 300 K

V2 (final volume) = ? (in L)

Now, we apply the data of the variables above to the General Equation of Gases, let's see:

$(P_1*V_1)/(T_1) =(P_2*V_2)/(T_2)$

$(12*23)/(200) =(14*V_2)/(300)$

$(276)/(200) =(14\:V_2)/(300)$

multiply the means by the extremes

$200*14\:V_2 = 276*300$

$2800\:V_2 = 82800$

$V_2 = \frac{82800\!\!\!\!\!\!\!\frac{\hspace{0.4cm}}{~}}{2800\!\!\!\!\!\!\!\frac{\hspace{0.4cm}}{~}}$

$V_2 \approx 29.57142857... \to \boxed{\boxed{V_2 \approx 30\:L}}\:\:\:\:\:\:\bf\blue{\checkmark}$

*** Note: the approximation rule says that when the number before the digit 5 is odd, the previous value is raised to the next even number

Answer:

The new volume is approximately 30 Liters

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Answers

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Explanation:

Answer:

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