Question

A 3.88 mol sample of gas has a temperature of 28°C and a pressure of 885 torr. What is its volume?

Answer 1

Answer:

V = 82.31L

Explanation:

Number of moles (n) = 3.88 moles

Temperature (T) = 28.0°C = (28.0 + 237.15)k = 301.15K

P = 885torr = 1.164atm (convert pressure in torr to atm)

1 atm = 760torr

x atm = 885 torr

X = (885 * 1) / 760

P = 1.164atm.

Volume (V) = ?

R = 0.082J/mol.K

From ideal gas equation,

PV = nRT

P = pressure

V = volume of the gas

n = number of moles

R = idealgas constant

T = temperature

PV = nRT

V = nRT/ P

V = (3.88 * 0.082 * 301.15) / 1.164

V= 82.31L

The volume of the gas is 82.31L

Answer 2

Answer:

Its volume is 82.3 L

Explanation:

The state of a quantity of gaseous matter is formulated based on four different variables: pressure, volume, temperature and number of moles of gas. Then, the equation known as the ideal gas equation, explains the relationship between these four variables using the expression:

P*V=n*R*T

where P represents the gas pressure, V its volume, n the number of moles of gas, R the gas constant and T the gas temperature.

In this case:

• P= 885 torr
• V=?
• n=3.88 mol

• R= 62.36365 $\frac{L*torr}{mol*K}$

• T=28°C= 301°K (Being 0°C=273°K)

Replacing:

885 torr*V=3.88 mol*62.36365 $\frac{L*torr}{mol*K}$*301°K

Solving:

$V=\frac{3.88mol*62.36365 \frac{L*torr}{mol*K} *301K}{885 torr}$

V=82.3 L

Its volume is 82.3 L