But-2-yne is reacted separately with one mole of Hydrogen as shown below:
A. A is more soluble than B
B. B The boiling point & melting point of $A$ are higher and lower than $B$ respectively
C. A is more polar than $B$ because dipole moment of $A$ is zero
D. $Br _2$ adds easily to $B$ than $A$
Identify the incorrect statements from the options given below:
A, C & D only
B, C & D only
The correct answer is option (C): B, C & D only
For hydrogen-like species, which of the following graphs provides the most appropriate representation of \( E \) vs \( Z \) plot for a constant \( n \)?
[E : Energy of the stationary state, Z : atomic number, n = principal quantum number]
Consider the following data:
- Heat of formation of \( CO_2(g) \) = -393.5 kJ mol\(^{-1}\)
- Heat of formation of \( H_2O(l) \) = -286.0 kJ mol\(^{-1}\)
- Heat of combustion of benzene = -3267.0 kJ mol\(^{-1}\)
The heat of formation of benzene is ……… kJ mol\(^{-1}\) (Nearest integer).
Which of the following is/are correct with respect to the energy of atomic orbitals of a hydrogen atom?
(A) \( 1s<2s<2p<3d<4s \)
(B) \( 1s<2s = 2p<3s = 3p \)
(C) \( 1s<2s<2p<3s<3p \)
(D) \( 1s<2s<4s<3d \)
Choose the correct answer from the options given below:
An ideal gas undergoes a cyclic transformation starting from point A and coming back to the same point by tracing the path A→B→C→D→A as shown in the three cases below.
Choose the correct option regarding \(\Delta U\):
Let a line passing through the point $ (4,1,0) $ intersect the line $ L_1: \frac{x - 1}{2} = \frac{y - 2}{3} = \frac{z - 3}{4} $ at the point $ A(\alpha, \beta, \gamma) $ and the line $ L_2: x - 6 = y = -z + 4 $ at the point $ B(a, b, c) $. Then $ \begin{vmatrix} 1 & 0 & 1 \\ \alpha & \beta & \gamma \\ a & b & c \end{vmatrix} \text{ is equal to} $
Resonance in X$_2$Y can be represented as
The enthalpy of formation of X$_2$Y is 80 kJ mol$^{-1}$, and the magnitude of resonance energy of X$_2$Y is:
Dihydrogen is the homonuclear diatomic molecule built from two hydrogen atoms. This molecule characterizes a covalent bond between two hydrogen atoms, satisfying each of their required pair configurations.
The dihydrogen molecule characterizes a single covalent bond between the two hydrogen atoms that comprise it. This molecule has a linear shape and is nonionic in nature. Each hydrogen atom comes up with one electron towards the covalent bond.