In which of the following reactions has the oxidation number of nitrogen increased?
2NO(g) + Br2(l) → 2NOBr(l)
2NO(g) + O2(g) → 2NO2(g)
FeSO4(aq) + NO(g) → Fe(NO)SO4(s)
2NO(g) + Cl2(g) → 2NOCl(l)
Correct answer is B
No explanation has been provided for this answer.
As the concentration of an electrolyte reduces, the conductivity
reduces to zero
decreases
increase
is unaffected
Correct answer is C
No explanation has been provided for this answer.
When ΔH is negative, a reaction is said to be
ionic
reversible
exothermic
endothermic
Correct answer is C
No explanation has been provided for this answer.
3Cu(s) + 8HNO3(aq) 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g)
In the equation above, copper is
an electron acceptor
a base
an oxidizing agent
a reducing agent
Correct answer is D
A reducing agent (also called a reductant or reducer) is an element or compound that loses (or "donates") an electron to another chemical species in a redox chemical reaction. Since the reducing agent is losing electrons, it is said to have been oxidized. In the reaction, Copper is oxidized.
decreasing the temperature of the system
Increase the pressure of the system
The addition of a catalyst to the system
Increasing the surface area of the vessel
Correct answer is A
Decrease in temperature favors in Equilibrium Constant[k] for this exothermic reaction.