Question

	Column I		Column II
a.	Temperature of a system always decreases	p.	$C{H}_2=CH-CH=C{H}_2$
b.	${\left(\begin{array}{c}\frac{\partial U}{\partial V}\end{array}\right)}_T=0$	q.	Internal energy increases
c.	Temperature of the system increases	r.	Ideal gas
d.	$\Delta H_{hydrogenation\left(experimental\right)}$ $<\Delta H_{hydrogenation\left(calculated\right)}$	s.	Adiabatic expansion

• A. $(a\to p)$
  $(b\to q)$
  $(c\to s)$
  $(d\to r)$
• B. $(a\to q)$
  $(b\to r)$
  $(c\to p)$
  $(d\to s)$
• C. $(a\to s)$
  $(b\to r)$
  $(c\to q)$
  $(d\to p)$
• D. $(a\to r)$
  $(b\to q)$
  $(c\to s)$
  $(d\to p)$

Answer 1

Answer: (C)

$(a\to s)$

$(b\to r)$
$(c\to q)$
$(d\to p)$

(a) Adiabatic expansion against pressure, or a spring causes a drop in temperature.

(b) For an ideal gas, ${\left(\frac{\partial U}{\partial V}\right)}_T=0,dV=C_{V}dT$ for all processes, $dq=dU+PdV$

(c) For ideal gas internal energy is directly proportional to its temperature, therefore its internal energy always increases with increase in temperature.

(d) For 1,3-butadiene $(C{H}_2=CH-CH=C{H}_2)$ upon hydrogenation

$△H_{\left(experimental\right)}<△H_{\left(calculated\right)}$