Answer:
ΔS=0.148 KJ/K
Explanation:
Given that
Q = 100 KJ
T₁=200°C
T₁=200+273 = 437 K
T₂=5°C
T₂=5 + 273 = 278 K
Reservoir 1 is rejecting heat that is why it taken as negative while the reservoir 2 is gaining the heat that is why it is taken as positive.
So the total change in entropy given as
ΔS= - Q/T₁ + Q/T₂
ΔS= - 100/473 + 100/278 KJ/K
ΔS=0.148 KJ/K
Answer:
Explanation:
1. Temperature of the bottle when only helium gas was present :T
P= 1.83 atm
V = 2.50 L
n = 0.458 moles
Using an Ideal gas equation:
PV=nRT
T= PV/nR= 1.83*2.50/0.458* 0.0821 =121.81K
2. Temperature of the bottle when argon gas is added into the container:T'
P' =2.05 atm
V = 2.50 L
n' = 0.458 mol + 0.713 mol = 1.171 mol
PV=nRT
T= PV/nR = 1.83*2.50/1.171*0.0802 = 53.37
The change in temperature will be
Final temperature = Initial temperature:T' - T
53.37 k - 121.81 K = -68.44 K
The change in temperature of the gas mixture is -68.44 K.
Answer:
Mass = 3.84 g
Explanation:
Given data:
Mass of hydrogen sulfide = 2.7 g
Mass of oxygen required = ?
Solution:
Chemical equation:
2H₂S + 3O₂ → 2H₂O + 2SO₂
Number of moles of hydrogen sulfide:
Number of moles = mass/ molar mass
Number of moles = 2.7 g / 34 g/mol
Number of moles = 0.08 mol
Now we will compare the moles of hydrogen sulfide with oxygen.
H₂S : O₂
2 : 3
0.08 : 3/2 ×0.08 = 0.12 mol
Mass of oxygen;
Mass = number of moles × molar mass
Mass = 0.12 mol × 32 g/mol
Mass = 3.84 g
Answer:
either element or pure substance but i think its element
Explanation:
