Respuesta :
Answer:
The pressure will be 0,37 atm.
Explanation:
We use the Boyle Mariotte´s formula,where for a given mass of gas, at constant temperature, the pressure and temperature vary inversely proportionally. We see here that the initial and final temperature does not vary (298K).
We convert the unit Celsius into Kelvin (0 ° C = 273K) and the unite mmHg into atm (760mmHg=1 atm):
25°C= 25+273=298K ; (1060mmHgx 1 atm)/760mmHg)=1,39 atm.
We convert unit of volume from ml to L: 174/1000=0,174L and 650/1000=0,650L
P1xV1= P2xV2
1,39 atm x 0,174L =P2 x0,650L
P2= (1,39 atm x 0,174L)/0,650L= 0,37 atm
Answer:
The pressure of the gas will decrease to 275.7 mmHg or 0.362 atm
Explanation:
Step 1: Data given
Volume of methane = 174.0 mL = 0.174 L
Temperature = 25.0 °C = 298 K
Pressure = 1030 mmHg = 1030/760 atm = 1.355263 atm
Volume increases to 650.0 mL = 0.650 L
The temperature stays constant
Step 2: Calculate the new pressure
P1*V1 = P2*V2
⇒with P1 = the initial pressure = 1.355263 atm
⇒with V1 = the initial volume = 0.174 L
⇒with P2 = the new pressure = TO BE DETERMINED
⇒with V2 = the new volume = 0.650 L
1.355263 * 0.174 = P2 * 0.650
P2 = 0.362 atm = 275.7 mmHg
OR
1030*0.174 = P2 * 0.650
P2 = 275.7 mmHg
The pressure of the gas will decrease to 275.7 mmHg or 0.362 atm
