A sample of ammonia gas occupies 23.6 mL at 527 mm Hg and 24.6oC. If the volume of the gas is changed to 53.9 mL at 56.7oC, what is the new pressure?

The new pressure is 255.6 mmHg

Explanation:

Step 1:Data given

Volume of the ammonia gas = 23.6 mL = 0.0236 L

Pressure of the ammonia gas = 527 mmHg

The temperature is 24.6 °C = 297.75 K

The volume increases to 53.9 mL

The increases to 56.7 °C = 329.85 K

Step 2: Calculate the new pressure

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

⇒with P1 = the initial pressure ofammonia gas = 527 mmHg

⇒with V1 = the initial Volume of ammonia gas = 23.6 mL = 0.0236 L

⇒with T1 = the initial temperature = 297.75 K

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume = 0.0539 L

⇒with T2 = the increased temperature = 329.85 K

527 mmHg * 0.0236 L  / 297.75 K  =  P2* 0.0539 L / 329.85 K

0.04177 = P2* 0.0539 L / 329.85 K

P2 * 0.0539 = 13.778

P2 = 255.6 mmHg

The new pressure is 255.6 mmHg

the answer is na (sodium)