Question

If the partial pressure of a gas produced in a reaction was determined to be 0.35 atm in a 161.0 ml container and at a temperature of 25.0°c, how many moles of gas were produced?

Answer 1

Answer: The number of moles of gas produced are 0.0023 moles.

Explanation:

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

$PV=nRT$

where,

P = pressure of the gas = 0.35 atm

V = Volume of the gas = 161.0 mL = 0.161 L    (Conversion factor: 1 L = 1000 mL)

T = Temperature of the gas = $25^oC=[25+273]K=298K$

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

n = number of moles of gas = ?

Putting values in above equation, we get:

$0.35atm\times 0.161L=n\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 298K\\\\n=\frac{0.35\times 0.161}{0.0821\times 298}=0.0023mol$

Hence, the number of moles of gas produced are 0.0023 moles.

Answer 2

Thank you for posting your question here at brainly. I hope the answer will help you. The number of moles of gas were produced the answer will be 0.0023 mol. 

Feel free to post your question here at brainly, if you have more questions.