Objective Questions

Questions (1872)

#	Question	Topic	Actions
701	What is the SI unit of specific heat capacity (Cs)?	CHM 101 Past Questions	View
702	Which of the following is an extensive property?	CHM 101 Past Questions	View
703	Which of the following characteristics describe an endothermic reaction?	CHM 101 Past Questions	View
704	Select all statements that are consistent with the First Law of Thermodynamics:	CHM 101 Past Questions	View
705	Which of the following forms of molecular motion contribute to the kinetic ener…	CHM 101 Past Questions	View
706	Why does diamond not spontaneously convert into graphite at room temperature de…	CHM 101 Past Questions	View
707	What is the specific effect of introducing a catalyst into a nonspontaneous the…	CHM 101 Past Questions	View
708	Which endothermic process provides clear evidence that enthalpy release is not …	CHM 101 Past Questions	View
709	Which statement correctly describes a reversible thermodynamic process?	CHM 101 Past Questions	View
710	Who introduced the thermodynamic property 'entropy' and its original concept in…	CHM 101 Past Questions	View
711	For an isothermal process, what is the thermodynamic definition of the entropy …	CHM 101 Past Questions	View
712	In Boltzmann's formulation S = k ln(W), what physical quantity does the paramet…	CHM 101 Past Questions	View
713	How does Ludwig Boltzmann's expression define the entropy change between an ini…	CHM 101 Past Questions	View
714	Which of the following molecular motions contribute to the thermal energy and m…	CHM 101 Past Questions	View
715	Which of the following correctly orders the standard molar entropies of the phy…	CHM 101 Past Questions	View
716	Which of the following conditions lead to an increase in the entropy of a syste…	CHM 101 Past Questions	View
717	According to the Second Law of Thermodynamics, what occurs to the entropy of th…	CHM 101 Past Questions	View
718	At constant temperature and pressure, how is the entropy change of the surround…	CHM 101 Past Questions	View
719	Why does a given exothermic heat release produce a much larger increase in Delt…	CHM 101 Past Questions	View
720	How is the change in Gibbs free energy (Delta G) related to the entropy change …	CHM 101 Past Questions	View
721	What is the primary thermodynamic convenience of using Gibbs free energy rather…	CHM 101 Past Questions	View
722	According to the Third Law of Thermodynamics, what is the entropy of a pure, pe…	CHM 101 Past Questions	View
723	What is the relationship between the reaction quotient Q, the equilibrium const…	CHM 101 Past Questions	View
724	If a reaction mixture has Q < K, what are the sign of Delta G and the direction…	CHM 101 Past Questions	View
725	In the Haber process (N2(g) + 3 H2(g) 2 NH3(g)), what happens when excess NH3 i…	CHM 101 Past Questions	View
726	Why does a gas spontaneously expand to fill an evacuated container uniformly?	CHM 101 Past Questions	View
727	At temperatures below 0 °C, liquid water freezes spontaneously. What drives thi…	CHM 101 Past Questions	View
728	Which of the following element is a group I element?	CHM 101 Past Questions	View
729	The kinetic energy of a 7.3 kg steel ball traveling at 18.0 m/s ______ J.	CHM 101 Past Questions	View
730	Thermodynamics is the study of energy as it changes from one form to another, a…	Thermochemistry	View
731	A __________ is the specific part of the universe being studied.	Thermochemistry	View
732	A system that cannot exchange energy or matter is called __________.	Thermochemistry	View
733	A __________ system can exchange energy but not matter.	Thermochemistry	View
734	An __________ system can exchange both matter and energy.	Thermochemistry	View
735	Energy is the capacity to do work or transfer __________.	Thermochemistry	View
736	The energy of motion is called __________ energy, given by the formula T = 1/2 …	Thermochemistry	View
737	In chemistry, kinetic energy of atoms increases with __________.	Thermochemistry	View
738	__________ energy is stored due to an object's position or state.	Thermochemistry	View
739	In chemistry, the most important form of potential energy is __________ potenti…	Thermochemistry	View
740	Gravitational potential energy is given by __________.	Thermochemistry	View
741	Radiant energy from the sun is the primary __________ source for Earth.	Thermochemistry	View
742	Vegetation captures radiant energy through __________.	Thermochemistry	View
743	Chemical energy is a form of __________ energy stored in substances.	Thermochemistry	View
744	Chemical energy is released, stored, or converted during __________.	Thermochemistry	View
745	The SI unit for energy is the __________ (J).	Thermochemistry	View
746	Another common unit is the __________ (cal).	Thermochemistry	View
747	1 cal = __________ J.	Thermochemistry	View
748	A person weighing 75.0 kg running at 1.78 m/s has a kinetic energy of _________…	Thermochemistry	View
749	A 1360 kg car 36.6 m high has a gravitational potential energy of __________ kJ.	Thermochemistry	View
750	Work is energy used to move an object against a __________.	Thermochemistry	View
751	__________ is the amount of heat required to raise a substance's temperature by…	Thermochemistry	View
752	Specific heat capacity is per unit __________.	Thermochemistry	View
753	Molar heat capacity is per unit __________.	Thermochemistry	View
754	Expanding a gas from 46 L to 64 L against 15 atm does __________ J of work.	Thermochemistry	View
755	Heating 15.0 g of water from 20.0°C to 50.0°C requires __________ kJ of heat.	Thermochemistry	View
756	An __________ process absorbs heat; q is positive.	Thermochemistry	View
757	An __________ process releases heat; q is negative.	Thermochemistry	View
758	In an endothermic reaction, the energy of products is __________ than reactants.	Thermochemistry	View
759	Internal energy (U) is the total __________ and potential energy of a system.	Thermochemistry	View
760	It increases with particle motion due to rising __________.	Thermochemistry	View
761	Internal energy is a __________ function.	Thermochemistry	View
762	The change in internal energy is ΔU = U_final - U_initial.	Thermochemistry	View
763	The first law states energy cannot be __________ or destroyed.	Thermochemistry	View
764	For a closed system, ΔU = __________.	Thermochemistry	View
765	For an endothermic process with q = +15.6 kJ and w = +1.4 kJ, ΔU = __________ k…	Thermochemistry	View
766	Compressing a gas with heat loss results in ΔU = __________ J.	Thermochemistry	View
767	Enthalpy (H) is defined as H = U + __________.	Thermochemistry	View
768	At constant pressure, ΔH = __________.	Thermochemistry	View
769	Enthalpy is a __________ function.	Thermochemistry	View
770	If H_products > H_reactants, the reaction is __________.	Thermochemistry	View
771	ΔH_rxn = Σ H_products - Σ H_reactants.	Thermochemistry	View
772	A balanced equation showing enthalpy change is a __________ equation.	Thermochemistry	View
773	For CS2(l) + 3O2(g) -> CO2(g) + 2SO2(g), ΔH° = __________ kJ/mol.	Thermochemistry	View
774	Burning 4.50 g of methane releases __________ kJ of heat.	Thermochemistry	View
775	For H2(g) + 1/2 O2(g) -> H2O(l), ΔH = __________ kJ.	Thermochemistry	View
776	Reversing 2H2O(l) -> 2H2(g) + O2(g) gives ΔH = __________ kJ.	Thermochemistry	View
777	The principle is: Heat lost = Heat __________.	Thermochemistry	View
778	A constant-volume calorimeter is called a __________ calorimeter.	Thermochemistry	View
779	The specific heat of water at 298 K is __________ J/g·K.	Thermochemistry	View
780	The specific heat of iron is __________ J/g·K.	Thermochemistry	View
781	In solution calorimetry, q = m × C_s × ΔT, where C_s for water is __________ J/…	Thermochemistry	View
782	A bomb calorimeter measures change in __________ energy (ΔU).	Thermochemistry	View
783	The specific heat of the metal calculated is __________ J/g·°C.	Thermochemistry	View
784	The enthalpy change for the neutralization reaction is __________ kJ/mol HCl.	Thermochemistry	View
785	Hess's Law states that the total enthalpy change is independent of the ________…	Thermochemistry	View
786	It relies on enthalpy being a __________ function.	Thermochemistry	View
787	For C(s) + 1/2 O2(g) -> CO(g), ΔH = __________ kcal/mol.	Thermochemistry	View
788	For N2O4(g) -> 2NO2(g), ΔH = __________ kcal.	Thermochemistry	View
789	Standard enthalpy of formation (ΔH_f°) is for the formation of __________ mole …	Thermochemistry	View
790	The standard enthalpy of formation for any element in its most stable form is _…	Thermochemistry	View
791	ΔH_f° for CO2(g) is __________ kJ/mol.	Thermochemistry	View
792	ΔH_f° for H2O(l) is __________ kJ/mol.	Thermochemistry	View
793	For NH3(g) + HCl(g) -> NH4Cl(s), ΔH_rxn = ΔH_f(NH4Cl) - ΔH_f(NH3) - ΔH_f(HCl).	Thermochemistry	View
794	The energy value of a fuel is often measured in __________ per kg.	Thermochemistry	View
795	Methane has a calorific value of __________ MJ/kg.	Thermochemistry	View
796	Hydrogen produces only __________ vapor when burned cleanly.	Thermochemistry	View
797	For a reaction to represent ΔH_f°, it must form __________ mole of compound fro…	Thermochemistry	View
798	The equation for the standard enthalpy of formation of liquid CCl4 is: ________…	Thermochemistry	View
799	Two small spheres carry charges of $0.0002 \text{ C}$ and $0.0004 \text{ C}$. I…	Thermochemistry	View
800	An electron (charge $\approx -1.6 \times 10^{-19} \text{ C}$) and a proton (cha…	Thermochemistry	View

Page 8 of 19

Quick Actions

Practice

Learning Tools

Stats & Progress

Community

Questions (1872)