Answer:
D) ΔU = -153.43 kJ and ΔH = -146.00 kJ
Explanation:
Given;
heat energy released by the exothermic reaction, ΔH = -146 kJ
number of gas mol, n = 3 mol
temperature of the gas, T = 298 K
Apply first law of thermodynamic
Change in the internal energy of the system, ΔU;
ΔU = ΔH- nRT
where;
R is gas constant = 8.314 J/mol.K
ΔU = -146kJ - (3 x 8.314 x 298)
ΔU = -146kJ - 7433 J
ΔU = -146kJ - 7.433 kJ
ΔU = -153.43 kJ
Therefore, the enthalpy change of the reaction ΔH is -146 kJ and change in the internal energy of the system is -153.43 kJ
D) ΔU = -153.43 kJ and ΔH = -146.00 kJ
Answer:
Explanation:
from figure
taking summation of force in x direction be zero
.....1
taking summation of force in Y direction be zero
.........2
putting T value in equation 1
.........3
Water at 10 degree C has kinetic viscosity v = 1.3 \times 10^{-6} m^2/s
Reynold number
so for Re = cd is 0.072
degree
Answer:
a
Explanation:
A is the answers since pedmas
for parentheses exponents division multiplacation addition subtranction in that order
Answer:
PPF
Explanation:
Production Possibilities Frontier