Heat produced in calories by the combustion of one gram of carbon is called
The temperature of the system decreases in an:
For the isothermal expansion of an ideal gas:
In an isochoric process, the increased internal energy is:
In an isochoric process, ΔV=0.
Hence, work done PΔV = W = 0.
So, ΔE = q+0.
Hence, the increase in internal energy will be equal to heat absorbed by the system
Internal energy is an example of:
Internal energy, enthalpy, and entropy are state quantities because they describe quantitatively an equilibrium state of a thermodynamic system, irrespective of how the system arrived in that state.
The process in which no heat enters or leaves the system is termed as:
An adiabatic process occurs without transfer of heat or mass of substances between a thermodynamic system and its surroundings. In an adiabatic process, energy is transferred to the surroundings only as work.
If in a container neither mass and nor heat exchange occurs then it constitutes a
An isolated system neither shows exchange of heat nor matter with surroundings.
Which of the following is true for an adiabatic process:
A process that does not involve the transfer of heat or matter into or out of a system, so that Q = 0, is called an adiabatic process, and such a system is said to be adiabatically isolated.
Among the following, intensive property is:
An intensive property is a property of matter that does not change as the amount of matter changes. It is a bulk property, which means it is a physical property that is not dependent on the size or mass of a sample. In contrast, an extensive property is one that does depend on sample size.
For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, ΔU and W correspond to:
Bomb calorimeter is commonly used to find the heat of combustion of organic substances which consists of a sealed combustion chamber, called a bomb. If a process is run in a sealed container then no expansion or compression is allowed, so w = 0 and ∆U = q.
∆U < 0, w = 0
Which of the following expressions represent the first law of thermodynamics:
The first law of thermodynamics is a version of the law of conservation of energy, adapted for thermodynamic systems. The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but can be neither created nor destroyed. The first law is often formulated
ΔE = Q + W
At 270C one mole of an ideal gas is compressed isothermally and reversibly from a pressure of 2 atm to 10 atm. The value of ΔE and q are (R = 2):
Isothermally (at constant temperature) and reversible work.
at constant temperature , ΔE = 0
ΔE = Q + W,
Q = −W = −965.84 cal
The heat required to raise the temperature of a body by 1K is called:
Which of the following is true for the reaction:
at 1000C at one atmosphere:
Identify the correct statement regarding entropy:
Maximum entropy will be in which of the following:
Entropy of gases is highest.
If enthalpies of formation C2H4 (g), CO2 (g) and H2O (l) at 2500C and 1 atm. pressure be 52, –394 and –286 KJ mol–1 respectively. The enthalpy of combustion of C2H4 (g) will be:
Heat of neutralization of strong acid and weak base is:
The heat evolved in the combustion of methane is given by the following equations:
How many grams of methane would be required to produce 444.15 KJ of heat of combustion:
One gram sample of NH4NO3 is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by 6.12 K. The heat capacity of the system is 1.23 kJ/g/deg. What is the molar heat of decomposition for NH4NO3?