Answer:
V = 38.48 L
Explanation:
Given that,
No. of moles = 1.5 mol
Pressure, P = 700 torr
Temperature, T = 15°C = 288 K
We need to find the volume of the gas. The ideal gas equation is given by :
, R = L.Torr.K⁻¹.mol⁻¹
So, the required volume is equal to 38.48 L.
Answer:
-0.050 kJ/mol.K
Explanation:
- A certain reaction is thermodynamically favored at temperatures below 400. K, that is, ΔG° < 0 below 400. K
- The reaction is not favored at temperatures above 400. K, that is. ΔG° > 0 above 400. K
All in all, ΔG° = 0 at 400. K.
We can find ΔS° using the following expression.
ΔG° = ΔH° - T.ΔS°
0 = -20 kJ/mol - 400. K .ΔS°
ΔS° = -0.050 kJ/mol.K
Answer: V = 33.9 L
Explanation: We will use Charles Law to solve for the new volume.
Charles Law is expressed in the following formula. Temperatures must be converted in Kelvin.
V1 / T1 = V2 / T2 then derive for V2
V2 = V1 T2 / T1
= 35 L ( 308 K ) / 318 K
= 33.9 L
Answer:
58.32
Explanation:
The mass number is one mole and for Mg it is 24.306 for O it is 15.999 and for H it is 1.008. because O and H have 2, you multiply them by 2 and add all the numbers and it equals 58.32
Answer:
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Explanation:
