A gas sample has an initial volume of 55.2 mL, an initial temperature of 35.0 °C, and an initial pressure of 735 mm Hg. The volume is decreased to 48.8 mL and the temperature is increased to 72.5 °C. What is the final pressure?

The answer to your question is   P2 = 932.6 mmHg

Explanation:

Data

Volume 1 = V1 = 55.2 ml

Temperature 1 = T1 = 35°C

Pressure 1 = P1 = 735 mmHg

Volume 2 = V2 = 48.8 ml

Temperature 2 = T2 = 72.5°C

Pressure 2 = P2 = ?

Process

1.- Convert temperature to °K

Temperature 1 = 35 + 273 = 308 °K

Temperature 2 = 72.5 + 273 = 345.5°K

2.- Use the Combine gas law to solve this problem

               P1V1/T1 = P2V2/T2

-Solve for P2

               P2 = P1V1T2 / T1V2

-Substitution

               P2 = (735 x 55.2 x 345.5) / (308 x 48.8)

-Simplification

               P2 = 14017626 / 15030.4

-Result

               P2 = 932.6 mmHg

43.452

step-by-step explanation:

284 times .153 = 43.452

a mercury barometer is a device that uses the physical properties of mercury in a tube to measure barometric pressure. mercury barometers are used for : -

1. measurement of atmospheric pressure  

2. determining the altitude of a place

3. weather forecasting

4. calibration and checking of aneroid barometers

5. application in fluid mechanics

6. measurement of pressure in aircrafts

7. surface weather analysis

8. preparation of barographs

9. usage in physical sciences like physics, astronomy & chemistry

10. preparation of aircraft altimeters

characteristics of mercury barometer : -

1.used to define and measure atmospheric pressure.

2.on the average at sea level the column of mercury rises to a height of about 760 mm.

3.this quantity is equal to 1 atmosphere.

4.it is also known as standard atmospheric pressure.

5.a barometer in which the weight of a column of mercury in a glass tube with a sealed top is balanced against that of the atmosphere pressing on an exposed cistern of mercury at the base of the mercury column, the height of the column varying with atmospheric pressure.