Explanation:
As it is given that water level is same as outside which means that theoretically, P = 756.0 torr.
So, using ideal gas equation we will calculate the number of moles as follows.
PV = nRT
or, n = 
= 
= 0.0052 mol
Also, No. of moles = 
0.0052 mol = 
mass = 0.0104 g
As some of the water over which the hydrogen gas has been collected is present in the form of water vapor. Therefore, at
= 24 mm Hg
=
atm
= 0.03158 atm
Now, P = 
= 0.963 atm
Hence, n =
= 0.0056 mol
So, mass of
= 0.0056 mol × 2
= 0.01013 g (actual yield)
Therefore, calculate the percentage yield as follows.
Percent yield = 
=
= 97.49%
Thus, we can conclude that the percent yield of hydrogen for the given reaction is 97.49%.
The answer is 1.164451827 moles
Answer:
d. 60.8 L
Explanation:
Step 1: Given data
- Heat absorbed (Q): 53.1 J
- External pressure (P): 0.677 atm
- Final volume (V2): 63.2 L
- Change in the internal energy (ΔU): -108.3 J
Step 2: Calculate the work (W) done by the system
We will use the following expression.
ΔU = Q + W
W = ΔU - Q
W = -108.3 J - 53.1 J = -161.4 J
Step 3: Convert W to atm.L
We will use the conversion factor 1 atm.L = 101.325 J.
-161.4 J × 1 atm.L/101.325 J = -1.593 atm.L
Step 4: Calculate the initial volume
First, we will use the following expression.
W = - P × ΔV
ΔV = - W / P
ΔV = - 1.593 atm.L / 0.677 atm = 2.35 L
The initial volume is:
V2 = V1 + ΔV
V1 = V2 - ΔV
V1 = 63.2 L - 2.35 L = 60.8 L
Answer: an arithmetical multiplier for converting a quantity expressed in one set of units into an equivalent expressed in another.
Explanation: