If 3.21 mol of a gas occupies 56.2 L at 44*C and 793 torr, 5.29 mol of this gas occupies __________ L under these conditions.
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-How will I solve this using PV= nRT?
I tried using PV= nRT. By just plugging in the value and got 131 but the answer is around 92.6. Thanks
Something is wrong with the problem. I plugged into Google calculator and obtained 80 something for volume at those conditions and NOT 56.2L.
Now that you mention it, I checked and under those conditions , the first value should not be 3.21 mols. So I guess that why I was unable to get the correct answer for 5.29 mols.I think the point of the conditions was just to say that the condition for the change were the same. It is possible to conclude that since the conditionals were the same, the mol of the gas is proportional to volume. Thus n1/v1 = n2/v2? THanks
I think you are right.
If 3.21 mol of a gas occupies 56.2 L at 44°C and 793 torr, 5.29 mol of this gas occupies __________ L under these conditions.
Group of answer choices
14.7
61.7
478
92.6
30.9
The ANSWER IS 92.6
To solve this problem using the ideal gas law equation PV = nRT, you need to follow a step-by-step approach.
Step 1: Determine the known values:
Given:
n1 = 3.21 mol (initial number of moles)
V1 = 56.2 L (initial volume)
T1 = 44 °C = 44 + 273 = 317 K (initial temperature)
P1 = 793 torr (initial pressure)
Step 2: Convert the initial pressure to the appropriate unit:
The ideal gas law equation requires pressure to be in units of Pascals (Pa). Therefore, you need to convert torr to Pascals. One torr is equal to 1/760th of an atmosphere, and one atmosphere is equal to 101325 Pascals. So, to convert torr to Pascals, multiply the torr value by 101325/760.
P1 = 793 torr * (101325 Pa / 760 torr) = 105374.34 Pa
Step 3: Determine the constant R:
The ideal gas constant R has a value of 0.0821 L·atm/(mol·K), but since the units in the problem are in Pascals rather than atmospheres, we need to use a different value for R. The value of R that is suitable for Pascals is 8.314 J/(mol·K).
Step 4: Calculate the initial number of moles (n1) of the gas using the given volume, temperature, and pressure:
Using the ideal gas law equation: PV = nRT
n1 = (P1 * V1) / (R * T1)
= (105374.34 Pa * 56.2 L) / (8.314 J/(mol·K) * 317 K)
≈ 2.89 mol
Step 5: Calculate the final volume (V2) of the gas using the given number of moles, temperature, and pressure:
Using the rearranged ideal gas law equation: V2 = (n2 * R * T2) / P2
Given:
n2 = 5.29 mol (final number of moles)
T2 = T1 (since the temperature is constant)
P2 = P1 (since the pressure is constant)
V2 = (n2 * R * T2) / P2
= (5.29 mol * 8.314 J/(mol·K) * 317 K) / 105374.34 Pa
≈ 92.6 L
So, approximately 92.6 L of the gas will occupy under these conditions.
My calculator is on the blink but
PV = nRT and V = nRT/P. Use 793/760 for P and solve for V. Don't forget to use T in kelvin (273+56.2). R is 0.08206