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

In an experiment, a sphere of aluminium of mass $0.20 \mathrm{kg}$ is heated up to $150°\mathrm{C}$ . Immediately, it is put into water of volume $150 \mathrm{cc}$at ${27}^{\mathrm{o}}\mathrm{C}$ kept in a calorimeter of water equivalent to$0.025 \mathrm{kg}$ . The final temperature of the system is ${40}^{\mathrm{o}}\mathrm{C}$ . The specific heat of the aluminium is(take $4.2 \mathrm{Joule}=1 \mathrm{calorie}$ )

A copper ball of mass $100 \mathrm{g}$ is at a temperature $T$. It is dropped in a copper calorimeter of mass $100 \mathrm{g},$ filled with $170 \mathrm{g}$ of water at room temperature. Subsequently, the temperature of the system is found to be ${75}^{\text{o}} \mathrm{C}$. $T$ is given by:
(Given: room temperature = ${30}^{\text{o}}\mathrm{C}$, the specific heat of copper $=0.1\hspace{0.17em}\mathrm{cal} {{\mathrm{g}}^{-1}}^{\mathrm{o}}{\mathrm{C}}^{-1}$)

Liquids $\mathrm{A}$ and $\mathrm{B}$ are at $\text{30\hspace{0.17em}°C}$ and $\text{20\hspace{0.17em}°C}$, respectively. When mixed in equal masses, the temperature of the mixture is found to be $\text{26\hspace{0.17em}°C}$, The specific heats of $\mathrm{A}$ and $\mathrm{B}$ are in the ratio of $m:n$ , then minimum value of $m+n=$ ?

The time taken for a calorimeter containing $75 \mathrm{g}$ of water at $62°\mathrm{C}$ to $\mathrm{cool}$ to $58°\mathrm{C}$ is $9$ minutes. When the calorimeter contains $105 \mathrm{g}$ of water, it takes $12$ minutes to cool from $62°\mathrm{C}$ to $58°\mathrm{C}$. The water equivalent of the calorimeter is

Three containers $C_1, C_2$ and $C_3$ have water at different temperatures. The table below shows the final temperature $T$ when different amounts of water (given in liters) are taken from each container and mixed (assume no loss of heat during the process)

The value of $\theta$ (in ${}^{\circ }\mathrm{C}$ to the nearest integer) is .....................

Find the final temperature in the form $2x°\mathrm{C}$ of the system when $5 \mathrm{gm}$ steam at $100°\mathrm{C}$ is mixed with $31.50 \mathrm{gm}$ ice at $-20°\mathrm{C}.$ Take $S_{\mathrm{ice}}=S_{\mathrm{steam} }=0.5 \mathrm{cal} {\mathrm{gm}}^{-1} °{\mathrm{C}}^{-1}, S_{water }=1 \mathrm{cal} {\mathrm{gm}}^{-1} °{\mathrm{C}}^{-1}$ and the latent heat of fusion and vaporization as $80 \mathrm{cal} {\mathrm{gm}}^{-1}$ and $540 \mathrm{cal} {\mathrm{gm}}^{-1}$ respectively. Find the value of $x$.

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 $=540 \mathrm{cal} {\mathrm{g}}^{-1}$)

An electrically heated coil is immersed in a $Q$ calorimeter containing $360 \mathrm{gm}$ of water at $10°\mathrm{C}$. The coil consumes energy at the rate of $90 \mathrm{W}$. The water equivalent of calorimeter & coil is $40 \mathrm{gm}.$ The temperature of water after $10$$\min$ is-

If $x \mathrm{gm}$ of steam at $100°\mathrm{C}$ becomes water at $100°\mathrm{C}$ which converts $y \mathrm{gm}$ of ice at $0°\mathrm{C}$ into water at $100°\mathrm{C}$, then the ratio $\frac{x}{y}$ will be,

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 $50°\mathrm{C}:$

Find the temperature of the mixture of $1 \mathrm{kg}$ of ice at $0^o$$\mathrm{C}$ and $1 \mathrm{kg}$ of water at ${10}^o$$\mathrm{C}$.

What is the final temperature of the mixture of $540 \mathrm{g}$ of ice at $0^o$$\mathrm{C}$ and $540 \mathrm{g}$ of water at ${80}^o$$\mathrm{C}$.

Consider mixing $1.5 \mathrm{kg}$ of ice at $0 °\mathrm{C}$ with $2 \mathrm{kg}$ of water at $70 °\mathrm{C}$ in a container. The resulting temperature of the mixture is found to be $5 °\mathrm{C}$. Calculate the heat of fusion of ice.$(s_{\mathrm{water}}=4186\mathrm{ }\mathrm{J}\mathrm{ }{\mathrm{kg}}^{-1}\mathrm{ }{}_{\mathrm{ }}{}^{\mathrm{ }}\mathrm{K}^{-1}\mathrm{ })$

Under which of the following condition is the following statement defined?

"Calorie is defined as the amount of heat required to raise the temperature of  $1\mathit{ }\mathrm{gm}$ of water by $1^o\mathrm{C}$" 

One gram of ice at$0{ }^{\mathrm{o}}\mathrm{C}$and one gram of steam at $100{ }^{\mathrm{o}}\mathrm{C}$ is mixed in a container. Then the amount of uncondensed steam left out is 

Water equivalent of a calorimeter is:

The whole mixture in the calorimeter become ice if: