Question

Pressure exerted by 220 g of CO2 gas in 8.21 dm3 vessel at 27°C is 0 1 atm O 5 atm O 10 atm O 15 atm ​

Answer 1

Answer: 15 atm

Explanation: We will use ideal gas equation to find out the amount of pressure.

The Ideal gas equation - $PV = nRT$, here P= Pressure,

V= Volume = 8.21 dm3 = 8.21 L

T = 27+ 273 = 300K ( Temperature)

R = Universal Gas Constant = 0.0831 atm L-1 K-1 mol-1

n = no of moles = Given Mass/ Molar Mass = 220 /44 = 5 ( Molar mass of CO2 is 44)

Now putting all the values on the Ideal gas equation, we can easily calculate the pressure.

$PV= nRT$

⇒ 8.21× P = 5×0.0831×300

⇒ P = 124.65÷ 8.21

⇒ P = 15

Hence the amount of pressure extracted by the 220 gm CO2 gas is 15 atm

To know more about the topic

https://brainly.in/question/48137477

https://brainly.in/question/7480833

#SPJ3

Answer 2

Answer:  The pressure exerted by 220 g of CO2 gas in an 8.21 dm3 vessel at 27°C is approximately 1197 atm.

Explanation:

The pressure exerted by a gas is determined by the number of gas molecules in the container, the temperature of the gas, and the volume of the container. To determine the pressure of 220 grams of CO2 gas in an 8.21 dm3 vessel at 27°C, you would need to know the molar mass of CO2 and the ideal gas law constant, R.

Using the ideal gas law, the pressure of the CO2 gas can be calculated as follows:

Pressure (atm) = $(n * R * T) / V$

where n is the number of moles of CO2, R is the ideal gas law constant, T is the temperature in Kelvin, and V is the volume in liters.

To determine the number of moles of CO2, you would need to know the molar mass of CO2, which is 44.01 g/mol. Then, you can use the following conversion to determine the number of moles of CO2:

n (mol) = $220 g CO2 / 44.01 g/mol$ = 4.98 mol

To convert the temperature from Celsius to Kelvin, you can add 273.15 to the temperature in Celsius:

T (K) = 27°C + 273.15 = 300.15 K

To convert the volume from dm3 to liters, you can multiply the volume in dm3 by 0.001:

V (L) = 8.21 dm3 * 0.001 = 0.0082 L

Finally, you can plug the values for n, R, T, and V into the ideal gas law equation to determine the pressure of the CO2 gas:

Pressure (atm) = $(4.98 mol * 8.31 J/mol*K * 300.15 K) / 0.0082 L$= 1197 atm

Therefore, the pressure exerted by 220 g of CO2 gas in an 8.21 dm3 vessel at 27°C is approximately 1197 atm.

To know more visit-https://brainly.com/question/29640318

#SPJ3