Dry ice is solid carbon dioxide. A 1.65−g sample of dry ice is placed in an evacuated 3.93−L vessel at 23.0°C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas.

The pressure of the gas inside the vessel is 0.232 atm

Explanation:

To calculate the number of moles, we use the equation:

Given mass of carbon dioxide = 1.65 g

Molar mass of carbon dioxide = 44 g/mol

Putting values in above equation, we get:

To calculate the pressure of the gas, we use the equation given by ideal gas which follows:

PV=nRT

where,

P = pressure of the gas = ?

V = Volume of the gas = 3.93 L

T = Temperature of the gas =

R = Gas constant =

n = number of moles of gas = 0.0375 moles

Putting values in above equation, we get:

Hence, the pressure of the gas inside the vessel is 0.232 atm

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

am i too late?

explanation: