I really need help with the following question....
What is the volume, in liters, of 0.250 mol of hydrogen gas at 20 °C and 0.974 atm pressure?
I also would like to let you know that
before you can put the numbers into an equation and solve for the volume, you need to convert 20 °C to Kelvins. T = 20°C + 273 = a blank box with a K next to the box.
Also what would be the formula used to solve volume for this problem?
After you have plug in the data of the above question what do you get? Don't forget to round the answer by the hundredths place.
PV = nRT.
T is in Kelvin, R is 0.08206 L*atm/mol*K, V is liters and P is in atmospheres. n is the number of mols.
This looks like a problem I saw yesterday. Post your work if you want to check your answer.
To solve this question, you need to use the Ideal Gas Law equation, which is:
PV = nRT
Where:
P = pressure in atmospheres (0.974 atm in this case)
V = volume in liters (unknown)
n = number of moles of gas (0.250 mol of hydrogen gas in this case)
R = gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin (20 °C + 273 = 293 K)
To find the volume (V), we can rearrange the equation as:
V = (nRT) / P
Now let's plug in the values to calculate the volume:
V = (0.250 mol * 0.0821 L·atm/(mol·K) * 293 K) / 0.974 atm
By performing the calculation, the answer is approximately 7.48 liters. Remember to round the answer to the hundredth place, which makes it 7.48 liters.