A sample of gas with an initial volume of 28.4 Liters at a pressure of 725 mmHg and a temperature of 305 K is compressed to a volume of 14.8 Liters and warmed to a temperature of 375 Kelvin. What is the final pressure of the gas?

The final pressure of the gas is 1.71 * 10³ mmHg.

Based on the given information,  

•The initial volume of gas is 28.4 L.

•The initial pressure of the gas is 725 mmHg.

•The initial temperature given is 305 K.  

•The final volume of the gas is 14.8 L.

•The final temperature given is 375 K.

Now the final pressure of the gas can be determined using ideal gas equation,

Thus, the final pressure of the gas is 1.71 * 10³ mmHg.

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The final pressure is 2.25 atm or 1710 mm Hg

Explanation:

Step 1: Data given

The initial volume = 28.4 L

The initial pressure = 725 mm Hg ( = 725/760 atm) = 0.953947 atm

The initial temperature = 305 K

The new volume is 14.8 L

The new temperature = 375 K

Step 2: Calculate the new pressure

(P1*V1)/T1 = (P2*V2)/T2

⇒ with P1 = the initial pressure = 725 mmHg = 0.953947 atm

⇒ with V1 = the initial volume = 28.4 L

⇒ with T1  = The initial temperature = 305 K

⇒ with P2 = the new pressure = TO BE DETERMINED

⇒ with V2 = the new volume = 14.8 L

⇒ with T2 = the new temperature = 375 K

(0.953947 * 28.4)/305 = (P2 * 14.8)/375

P2 = 2.25 atm = 1710 mm Hg

The final pressure is 2.25 atm or 1710 mm Hg

1. 1 mole of anything contains 6.022x10^23 pieces  

d  

2. a  

3. c, number  

5. 1.24x10^24atoms / 6.022x10^23atoms/mole = 2moles h2 atoms  

6. fe2br3 mass = 2moles x mass fe + 3 moles x mass br  

molar mass = grams / number of moles = g/mole  

to find moles = g / molar mass  

to find mass = g = molar mass / moles