Principle of Calorimetry

Initially, a beaker has $100 \mathrm{g}$ of water at temperature $90 °\mathrm{C}$. Later another $600 \mathrm{g}$ of water at temperature $20 °\mathrm{C}$ was poured into the beaker. The temperature, $T\left(\text{in} °\mathrm{C}\right)$ of the water after mixing is

Initially, a beaker has $100 \mathrm{g}$ of water at temperature $90 °\mathrm{C}$. Later another $600 \mathrm{g}$ of water at temperature $20 °\mathrm{C}$ was poured into the beaker. The temperature, $T$ of the water after mixing is

Calorie is the unit of which physical quantity?

$1 \mathrm{cal}=$_____ $\mathrm{J}$

Calorie is the unit of which physical quantity?

SI unit of heat is kelvin and SI unit of temperature is joule.

What is the SI unit of heat?

One calorie is nearly equal to _____ $\mathrm{J}$.

A heater supplying constant power $P$ watts is switched ON at time $t=0 \min$ to raise the temperature of a liquid kept in a calorimeter of negligible heat capacity. A student records the temperature of the liquid $T\left(t\right)$ at equal time intervals. A graph is plotted with $T\left(t\right)$ on the $Y$-axis versus $t$ on the $X$-axis. Assume that there is no heat loss to the surroundings during heating. Then,

Steam at $100 °\mathrm{C}$ is passed into $1 \mathrm{kg}$ of water contained in a calorimeter at $9 °\mathrm{C}$ till the temperature of water and calorimeter is increased to $90 °\mathrm{C}$. The mass of the stean condensed is nearly
(Water equivalent of calorimeter $=0.1 \mathrm{kg}$ Specific heat of water $=1 \mathrm{cal} {\mathrm{g}}^{-1} °{\mathrm{C}}^{-1}$ Latent heat of vapourisation $=540 \mathrm{cal} {\mathrm{g}}^{-1}$)

Two tank $A$ and $B$ contain water at $20°\mathrm{C}$ and $80°\mathrm{C}$ respectively. The amount of water that must be taken from $A$ and $B$ to prepare $40 \mathrm{kg}$ of water at $50°\mathrm{C}:$

Match the Column (A) and Column (B)

Column (A) Column (B)

a. The heating of a body takes place by conduction

b. Heat transfer in solid b. Its volume expands

c. of steel heat c. Measured by thermometer

d On heating the solid d. The substance has a property

e specific heat y. is a good conductor.

The whole mixture in the calorimeter become ice if:

A solid is heated up and $\Delta \text{H}$ vs $\Delta \theta$($∆H :$Heat given, $∆\theta :$change in temperature) is plotted as shown in figure. Material exist in only one phase in-

$10 kg$of ice at $–5°C$ is kept in a large container of negligible heat capacity $1 kg$of steam at $110°C$ is passed over the container. The final temp of mixture when thermal equilibrium is attained:

[Specific Heat of ice$=$ $0.5 cal/gm°C;$

Specific Heat of steam $= 0.47 cal/gm°C$$;$ $$

Latent Heat of fusion $= 80 cal/gm$

$4 \mathrm{g}$ of steam at $100{ }^0\mathrm{C}$ is added to$20 \mathrm{g}$of water at $46{ }^0\mathrm{C}$ in a container of negligible mass. Assuming no heat is lost to the surrounding, the mass of water in the container at thermal equilibrium is (Latent heat of vaporisation$=540 \mathrm{cal}/\mathrm{gm}$, specific heat of water$=1 \mathrm{cal}/\mathrm{gm} º\mathrm{C}$)

$2 \mathrm{kg}$ ice at $–20°\mathrm{C}$ is mixed with $5 \mathrm{kg}$water at $20°\mathrm{C}$in an insulating vessel having negligible heat capacity. Calculate the final mass of water remaining in the container.

Given: specific heat of water $= 4.186 \mathrm{kJ} {\mathrm{K}}^{-1} {\mathrm{kg}}^{-1}$

Specific heat of  ice $= 2.092 \mathrm{kJ} {\mathrm{K}}^{-1} {\mathrm{kg}}^{-1}$

Latent heat of fusion of ice $= 334.7 \mathrm{kJ} {\mathrm{kg}}^{-1}$

Water of volume $2 \mathrm{L}$ in a container is heated with a coil of power $1 \mathrm{kW}$ at $27{ }^0\mathrm{C}$. The lid of the container is open and energy dissipates at rate of $160 \mathrm{J}/\mathrm{s}$. In how much time temperature will rise from $27{ }^0\mathrm{C}$ to $77{ }^0\mathrm{C}$ ? [Given specific heat of water is $4.2 \mathrm{kJ}/\mathrm{kg}$]

$80 \mathrm{gm}$ of water at ${30}^o\mathrm{C}$ is poured on a large block of ice at $0^{\mathrm{o}}\mathrm{C}$. The mass of ice that melts is:

Liquids $\mathrm{A}$ and $\mathrm{B}$ are at $30 °\mathrm{C}$ and $20 °\mathrm{C}$, respectively. When mixed in equal masses, the temperature of the mixture is found to be $26 °\mathrm{C}$, The specific heats of $\mathrm{A}$ and $\mathrm{B}$ are in the ratio of $m:n$, where $m$ and $n$ are integers, then find the minimum value of $m+n$.