Question

11. A 5.73-L flask at 25 °C contains 0.0388 mol of N2.0.147 mol of Co, and 0.0803 mol of Hz.

What is the total pressure in the flask in atmospheres?​

Answer 1

The total pressure in the 5.73-L flask at 25 °C containing different amounts of N₂, CO, and H₂ is calculated to be 1.1307 atmospheres using the ideal gas law.

Step-by-step explanation:

To calculate the total pressure in the flask, we use the ideal gas law, which states that PV = nRT, where P is pressure, V is volume, n is number of moles, R is the ideal gas constant (0.0821 L\u00b7atm/K\u00b7mol), and T is the temperature in Kelvin. The temperature must be converted to Kelvin by adding 273.15 to the Celsius temperature.

First, convert the temperature to Kelvin: 25 °C + 273.15 = 298.15 K.
Next, sum up the total moles of gas: 0.0388 mol N₂ + 0.147 mol CO + 0.0803 mol H₂ = 0.2661 mol.

Now, use the ideal gas law to find the pressure (P):
P = (nRT) / V
P = (0.2661 mol × 0.0821 L\u00b7atm/K\u00b7mol × 298.15 K) / 5.73 L
P = 1.1307 atm (rounded to four significant figures)

Therefore, the total pressure in the flask is 1.1307 atmospheres.

Answer 2

`\large \boxed{\text{1.14 atm}}`

Step-by-step explanation:

The identity of the gases doesn't matter. All we need is the total number of moles.

1. Total number of moles

N₂ 0.0388 mol

CO 0.147

H₂ 0.0802

0.266 mol

2. Other data

V = 5.73 L

T = 25 °C

3. Total pressure

We can use the Ideal Gas Law:

pV = nRT

Calculations:

(a) Convert the temperature to kelvins

T = (25 + 273.15) K = 298.15 K

(b) Calculate the pressure

`\begin{array}{rcl}pV & =& nRT\\p * \text{5.73 L} & = & \text{0.266 mol} * \text{0.082 06 L$\cdot$ atm$\cdot$K$^(-1)$mol$^(-1)*$ 298.15 K}\\5.73p & = & \text{6.361 atm}\\p & = & \textbf{1.14 atm}\end{array}\\\text{The total pressure in the flask is $\large \boxed{\textbf{1.14 atm}}$}`