Question 4 :
When you combust $100.0\ g$ of propane at $500.K$ and $1.00\ atm$ in a closed container, you expected to collect $279\ L$ of carbon dioxide. Instead, when you collect the gas, it measures $651\ L$ in total.<br>Why have you collected more than your predicted, theoretical yield?

Question 6 :
For a reaction to be spontaneous in neither direction, which of the following is/are correct regarding the closed system?<br>(1) ${ \left( \Delta { G } \right) }_{ T,P }=0$<br>(2)${ \left( \Delta { G } \right) }_{ T,P }&lt; 0$<br>(3) ${ \left( \Delta { G } \right) }_{ U,V }=0$<br>(4) ${ \left( \Delta { G } \right) }_{ U,V }&gt;0$<br>Codes:

Question 7 :
Magnitude of Seebeck emf between the junctions does not depend on

Question 8 :
The following two equilibria exist simultaneously in a closed vessel :<br/>$PCI_5(g) \rightleftharpoons PCI_3(g) + Cl_2(g)$<br/>$COCI_2(g) \rightleftharpoons CO (g) + CI_2 (g)$<br/>If some CO is added into the vessel, then after the equlibrium is attained again, concertration of ?

Question 11 :
If there were no atmosphere, the average temperature on earth surface would be<br>

Question 12 :
An isolated system is one which neither shows an exchange of ____nor ____with surroundings.

Question 17 :
For the gas phase exothermic reaction, $A_2+B_2&#160;\rightleftharpoons C_2$, carried out in a closed vessel, the equilibrium moles of $A_2$, can be increased by :&#160;

Question 21 :
An open system can exchange both matter and energy with surroundings.<br/>

Question 24 :
In thermodynamic equilibrium there are no net &#160;____________ flows of matter or of energy, either within a system or between systems.

Question 25 :
Assertion: Water drops take spherical shape when falling freely. Reason: Water has minimum surface tension among all liquids.

Question 28 :
Assertion: Diamond is thermodynamically less stable than its allotrope graphite. Reason: Molar entropy of graphite is greater than that of diamond under similar conditions.

Question 29 :
Conversion of sulphur to $SO_3$ has $\triangle H=2xK cal$ and conversion of $SO_2$ to $SO_3$ involves $\triangle H=-ykcal$. The correct thermochemical equation for formation of $SO_2$ is:

Question 30 :
Which of the following parameters does not charaterize the thermodynamic state of matter?

Question 31 :
In a closed system : $A\left( s \right) \rightleftharpoons 2B\left( g \right) +3C\left( g \right) $ if the partial pressure C is of doubled then partial pressure B wil be:

Question 33 :
The value of -$\log K$ for a reaction :<br/>&#160; &#160; &#160; &#160; $A(g) \rightleftharpoons B(g)$<br/>[Given: $\Delta _r H^o _{298k} = -54.07kJ\,mol^{-1}, \Delta _r S^o_{298K}=-191.62kJ/K$&#160; &#160;and $2.303\times 8.314\times 298 = 5705$]

Question 34 :
A system in thermodynamic equilibrium will have the maximum value for :&#160;<br/>

Question 36 :
A system in thermodynamic equilibrium will have the minimum value for-? <br>

Question 37 :
Two reactions involving water are shown.<br>X anhydrous cobalt (II) chloride + water $\rightarrow$ hydrated cobalt(II) chloride<br>Y iron + oxygen + water $\rightarrow$ rust<br>Which reactions are reversible by heating?

Question 38 :
The value closest to the thermal velocity of a Helium atom at room temperature (300 K) in $ms^{-1}$ is : [$k_B = 1.4 \times 10^{-23} \ J/K ; \ m_{He} = 7\times 10^{-27} \ kg$ ]

Question 41 :
In a laboratory, liquid in a thermally insulated container is stirred for one hour by a mechanical linkage to a stirrer, for this process:

Question 42 :
"Heat cannot by itself flow from a body at lower temperature to a body at higher temperature" is a statement of the consequence of

Question 43 :
A child bought a balloon which became very small in size the next day. Which is correct statement about&#160;balloon?

Question 45 :
<p class="wysiwyg-text-align-left">The internal energy change when a system goes from state $A$ to $B$ is $40 \ kJmole^{-1}$. If the system goes from $A$ to $B$ by a reversible path and returns to state $A$ by an irreversible path, what would be the net change in internal energy?</p>

Question 46 :
In an evacuated closed isolated chamber at ${250}^{o}C$. $.02$ mole $P{Cl}_{5}$ and $.01$ mole ${Cl}_{2}$ are mixed $(P{Cl}_{5}\rightleftharpoons P{Cl}_{3}+{Cl}_{2})$. At equilibrium density of mixture was $2.49g/L$ and pressure was $1$ atm. The number of total moles at equilibrium will be approximately:

Question 47 :
Water of mass $m_2$ = 1 kg is contained in a copper calorimeter of mass&#160;$m_1$&#160;&#160;= 1 kg. Their common temperature&#160;t = $10^{0}C$. Now a piece of ice of mass&#160;$m_3$&#160;&#160;= 2 kg and temperature is $-11^{0}C$&#160;dropped into the calorimeter.&#160;Neglecting any heat loss, the final temperature of system is. [specific heat of copper = 0.1 Kcal/ kg$^{0}C$, specific&#160;heat of water = 1 Kcal/kg$^{0}C$, specific heat of ice = 0.5 Kcal/kg$^{0}C$, latent heat of fusion of ice = 78.7 Kcal/kg]

Question 48 :
Calculate the amount of ice that will separate out on cooling a solution containing $50$ g of ethylene glycol in $200$g of water to $-9.3&#176;C$.Molal depression constant for water is $1.86$ K kg/mol

Question 49 :
Two closed vessel $A$ and $B$ of equal volume of $8.21L$ are connected by a narrow tube of negligible volume with open valve. The left hand side container id found to contain $3\ mole \, CO_2$ and $2\ mole$ of $He$ at $400K$. What is the partial pressure of $He$ in vessel $B$ at $500K$?