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GRE Subject Test: Chemistry : Heat and Temperature

Study concepts, example questions & explanations for GRE Subject Test: Chemistry

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1 Diagnostic Test 152 Practice Tests Question of the Day Flashcards Learn by Concept

Example Questions

Example Question #1 : Heat And Temperature

Use the following values for water as needed.

$\Delta H^o_{fus}=334\frac{J}{g}$ $\displaystyle \Delta H^o_{fus}=334\frac{J}{g}$

$\Delta H^o_{vap}=2260\frac{J}{g}$ $\displaystyle \Delta H^o_{vap}=2260\frac{J}{g}$

$c=4.186\frac{J}{g^oC}$ $\displaystyle c=4.186\frac{J}{g^oC}$

$\rho = 1\frac{g}{mL}$ $\displaystyle \rho = 1\frac{g}{mL}$

If burning wood releases $\small 20kJ$ $\displaystyle \small 20kJ$ of heat energy per gram of wood consumed, what mass of wood must be consumed to heat $\small 1L$ $\displaystyle \small 1L$ of water from $\small 20^oC$ $\displaystyle \small 20^oC$ to $\small 100^oC$ $\displaystyle \small 100^oC$ , and then to convert it to water vapor?

Possible Answers:

134g $\displaystyle 134g$

2595g $\displaystyle 2595g$

17g $\displaystyle 17g$

335g $\displaystyle 335g$

130g $\displaystyle 130g$

Correct answer:

130g $\displaystyle 130g$

Explanation:

There are two processes requiring added heat in this problem:

1. Raising the temperature of the liquid water from $\small 20^oC$ $\displaystyle \small 20^oC$ to $\small 100^oC$ $\displaystyle \small 100^oC$ (use $\Delta Q = mc\Delta T$ $\displaystyle \Delta Q = mc\Delta T$ )

2. Boiling the water at a constant temperature of $\small 100^oC$ $\displaystyle \small 100^oC$ (use $\Delta Q = m\Delta H^o_{vap}$ $\displaystyle \Delta Q = m\Delta H^o_{vap}$ )

To use either of these equation, we need to find the mass of the water using the relation between mass, density, and volume.

$m = \rho*V= 1\frac{g}{mL}*1000mL=1000g$ $\displaystyle m = \rho*V= 1\frac{g}{mL}*1000mL=1000g$

Use this mass with the given specific heat and temperatures to find the heat for part 1 of the process.

$\Delta Q = (1000g)(4.186\frac{J}{g^oC})(100^oC - 20^oC)=334,880J$ $\displaystyle \Delta Q = (1000g)(4.186\frac{J}{g^oC})(100^oC - 20^oC)=334,880J$

Then, use the mass with the given heat of vaporization to find the energy needed to convert the water to water vapor.

$\Delta Q =(1000g) (2260\frac{J}{g})= 2,260,000J$ $\displaystyle \Delta Q =(1000g) (2260\frac{J}{g})= 2,260,000J$

Sum the energies for step 1 and step 2.

$334,880 J + 2,260,000 J = 2,594,880J\approx 2,595kJ$ $\displaystyle 334,880 J + 2,260,000 J = 2,594,880J\approx 2,595kJ$

This is the total amount of energy needed from the burning wood. Use stoichiometry to find the grams of wood needed to produce this amount of energy.

$2595kJ*(\frac{1 g}{20kJ})=129.7g\approx 130g$ $\displaystyle 2595kJ*(\frac{1 g}{20kJ})=129.7g\approx 130g$

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Example Question #1 : Heat And Temperature

What was the final temperature of water if a 19 g $\displaystyle 19 g$ sample of water absorbs 810.5 J $\displaystyle 810.5 J$ of heat energy and heats up from $25^{o}C$ $\displaystyle 25^{o}C$ ? (specific heat of water is $4.18 \frac{J}{g^{o}C}$ $\displaystyle 4.18 \frac{J}{g^{o}C}$ )

Possible Answers:

$44^{o}C$ $\displaystyle 44^{o}C$

$25^{o}C$ $\displaystyle 25^{o}C$

$18^{o}C$ $\displaystyle 18^{o}C$

35^oC $\displaystyle 35^oC$

Correct answer:

35^oC $\displaystyle 35^oC$

Explanation:

Specific heat is the amount of heat needed to raise 1 gram of a substance by 1^oC. Calorimeters used for these types of experiments because they are designed to be well-insulated, so no heat is gained from or lost to the surroundings.

$Specific\ heat(C)=\frac{amount\ of\ heat\ transferred(Q)}{(grams\ of\ substance,m)\times (temperature\ change\bigtriangleup, T)}$ $\displaystyle Specific\ heat(C)=\frac{amount\ of\ heat\ transferred(Q)}{(grams\ of\ substance,m)\times (temperature\ change\bigtriangleup, T)}$

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

$Q=mC\bigtriangleup T$ $\displaystyle Q=mC\bigtriangleup T$

$Q=mC(T_{f}-T_{i})$ $\displaystyle Q=mC(T_{f}-T_{i})$

$810.5J=19g\times4.179\frac{J}{g^{o}C}\times(T_{f}-25^{o}C)$ $\displaystyle 810.5J=19g\times4.179\frac{J}{g^{o}C}\times(T_{f}-25^{o}C)$

$810.5J=79.40\frac{J}{^{o}C}\times(T_{f}-25^{o}C)$ $\displaystyle 810.5J=79.40\frac{J}{^{o}C}\times(T_{f}-25^{o}C)$

$\frac{810.5J}{79.40\frac{J}{^{o}C}}=T_{f}-25^{o}C$ $\displaystyle \frac{810.5J}{79.40\frac{J}{^{o}C}}=T_{f}-25^{o}C$

$10.21^{o}C=T_{f}-25^{o}C$ $\displaystyle 10.21^{o}C=T_{f}-25^{o}C$

$T_{f}=35^{o}C$ $\displaystyle T_{f}=35^{o}C$

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Example Question #1 : Heat And Temperature

An 81.9 g $\displaystyle 81.9 g$ metal at $54.2^{o}C$ $\displaystyle 54.2^{o}C$ was put into 40.7g $\displaystyle 40.7g$ of water at $25^{o}C$ $\displaystyle 25^{o}C$ . The final temp of the water and metal was $29.3^{o}C$ $\displaystyle 29.3^{o}C$ . Assuming heat was not lost to the surroundings find the specific heat of the metal? The specific heat of water is $4.18\frac{J}{g^{o}C}$ $\displaystyle 4.18\frac{J}{g^{o}C}$ .

Possible Answers:

$0.358\frac{J}{g^{o}C}$ $\displaystyle 0.358\frac{J}{g^{o}C}$

$4.8\frac{J}{g^{o}C}$ $\displaystyle 4.8\frac{J}{g^{o}C}$

$6.9\frac{J}{g^{o}C}$ $\displaystyle 6.9\frac{J}{g^{o}C}$

$2.4\frac{J}{g^{o}C}$ $\displaystyle 2.4\frac{J}{g^{o}C}$

Correct answer:

$0.358\frac{J}{g^{o}C}$ $\displaystyle 0.358\frac{J}{g^{o}C}$

Explanation:

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

Heat is transferred from the metal to the water.

$-Q_{metal}=Q_{water}$ $\displaystyle -Q_{metal}=Q_{water}$

$-(mC\bigtriangleup T)=mC\bigtriangleup T$ $\displaystyle -(mC\bigtriangleup T)=mC\bigtriangleup T$

$-(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$ $\displaystyle -(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$

$-(81.9g\cdot C\cdot (29.3^{o}C-54.2^oC)=40.7g\cdot4.18\frac{J}{g^o}C(29.3^{o}C-25^{o}C)$ $\displaystyle -(81.9g\cdot C\cdot (29.3^{o}C-54.2^oC)=40.7g\cdot4.18\frac{J}{g^o}C(29.3^{o}C-25^{o}C)$

$-(-2039g^{o}C\cdot C)=731J$ $\displaystyle -(-2039g^{o}C\cdot C)=731J$

$2039g^{o}C\cdot\ C=731J$ $\displaystyle 2039g^{o}C\cdot\ C=731J$

$C=\frac{731J}{2039g^{o}C}=0.358\frac{J}{g^{o}C}$ $\displaystyle C=\frac{731J}{2039g^{o}C}=0.358\frac{J}{g^{o}C}$

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Example Question #1 : Heat And Temperature

Calculate the final temperature when a 44.0g $\displaystyle 44.0g$ sample of metal (specific heat of the metal= $0.52 \frac{J}{g^{o}C}$ $\displaystyle 0.52 \frac{J}{g^{o}C}$ ) at $45.0^{o}C$ $\displaystyle 45.0^{o}C$ is placed into 95.0g $\displaystyle 95.0g$ of water at $23.0^{o}C$ $\displaystyle 23.0^{o}C$ . (specific heat of water is $4.18\frac{J}{g^{o}C}$ $\displaystyle 4.18\frac{J}{g^{o}C}$ )

Possible Answers:

$132^{o}C$ $\displaystyle 132^{o}C$

$76^{o}C$ $\displaystyle 76^{o}C$

$17^{o}C$ $\displaystyle 17^{o}C$

$24^{o}C$ $\displaystyle 24^{o}C$

Correct answer:

$24^{o}C$ $\displaystyle 24^{o}C$

Explanation:

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

Heat is transferred from the metal to the water.

$-Q_{metal}=Q_{water}$ $\displaystyle -Q_{metal}=Q_{water}$

$-(mC\bigtriangleup T)=mC\bigtriangleup T$ $\displaystyle -(mC\bigtriangleup T)=mC\bigtriangleup T$

$-(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$ $\displaystyle -(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$

$-(44.0g\cdot 0.52\frac{J}{g^{o}C}\cdot (T_{f}-45.0^oC)=95.0g\cdot4.18\frac{J}{g^o}C(T_{f}-23^{o}C)$ $\displaystyle -(44.0g\cdot 0.52\frac{J}{g^{o}C}\cdot (T_{f}-45.0^oC)=95.0g\cdot4.18\frac{J}{g^o}C(T_{f}-23^{o}C)$

$-(22.9\frac{J}{^{o}C}(T_{f}-45.0^{o}C))=397\frac{J}{^{o}C}(T_{f}-23^{o}C)$ $\displaystyle -(22.9\frac{J}{^{o}C}(T_{f}-45.0^{o}C))=397\frac{J}{^{o}C}(T_{f}-23^{o}C)$

$-(22.9\frac{J}{^{o}C}\cdot T_{f}-22.9\frac{J}{^{o}C}\cdot 45.0^{o}C)=397\frac{J}{^{o}C}\cdot T_{f}-397\frac{J}{^{o}C}\cdot 23.0^{o}C$ $\displaystyle -(22.9\frac{J}{^{o}C}\cdot T_{f}-22.9\frac{J}{^{o}C}\cdot 45.0^{o}C)=397\frac{J}{^{o}C}\cdot T_{f}-397\frac{J}{^{o}C}\cdot 23.0^{o}C$

$-(22.9\frac{J}{^{o}C}\cdot T_{f}-1031J)=397\frac{J}{^{o}C}\cdot T_{f}-9131J$ $\displaystyle -(22.9\frac{J}{^{o}C}\cdot T_{f}-1031J)=397\frac{J}{^{o}C}\cdot T_{f}-9131J$

$-22.9\frac{J}{^{o}C}\cdot \ T_{f}+1031J=397\frac{J}{^{o}C}\cdot T_{f}-9131J$ $\displaystyle -22.9\frac{J}{^{o}C}\cdot \ T_{f}+1031J=397\frac{J}{^{o}C}\cdot T_{f}-9131J$

$-22.9\frac{J}{^{o}C}\cdot \ T_{f}-397\frac{J}{^{o}C}\cdot T_{f}=-1031J-9131J$ $\displaystyle -22.9\frac{J}{^{o}C}\cdot \ T_{f}-397\frac{J}{^{o}C}\cdot T_{f}=-1031J-9131J$

$-419\frac{J}{^{o}C}\cdot T_{f}=-10162J$ $\displaystyle -419\frac{J}{^{o}C}\cdot T_{f}=-10162J$

$T_{f}=\frac{-10162^{o}C}{-419.9}=24^{o}C$ $\displaystyle T_{f}=\frac{-10162^{o}C}{-419.9}=24^{o}C$

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Example Question #1 : Heat And Temperature

Calculate the specific heat of 19.3 g $\displaystyle 19.3 g$ of metal that requires 353 J $\displaystyle 353 J$ of heat energy to raise its temperature from $17.0^{o}C$ $\displaystyle 17.0^{o}C$ to $44.0^{o}C$ $\displaystyle 44.0^{o}C$ ?

Possible Answers:

$0.677\frac{J}{g^{o}C}$ $\displaystyle 0.677\frac{J}{g^{o}C}$

$17\frac{J}{g^{o}C}$ $\displaystyle 17\frac{J}{g^{o}C}$

$0.581\frac{J}{g^{o}C}$ $\displaystyle 0.581\frac{J}{g^{o}C}$

$0.98\frac{J}{g^{o}C}$ $\displaystyle 0.98\frac{J}{g^{o}C}$

Correct answer:

$0.677\frac{J}{g^{o}C}$ $\displaystyle 0.677\frac{J}{g^{o}C}$

Explanation:

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

$C=\frac{Q}{m\bigtriangleup T}=\frac{353J}{(19.3g\times (44.0^{o}C-17.0^{o}C))}=0.677\frac{J}{g^{o}C}$ $\displaystyle C=\frac{Q}{m\bigtriangleup T}=\frac{353J}{(19.3g\times (44.0^{o}C-17.0^{o}C))}=0.677\frac{J}{g^{o}C}$

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Example Question #31 : Thermodynamics And Phases

What was the final temperature of the water if a 33.0 g $\displaystyle 33.0 g$ sample of water absorbs 423 J $\displaystyle 423 J$ of heat energy and heats up from $23^{o}C$ $\displaystyle 23^{o}C$ ? (specific heat of water is $4.18 \frac{J}{g^{o}C}$ $\displaystyle 4.18 \frac{J}{g^{o}C}$ )

Possible Answers:

$71^{o}C$ $\displaystyle 71^{o}C$

$54^{o}C$ $\displaystyle 54^{o}C$

$28^{o}C$ $\displaystyle 28^{o}C$

$117^{o}C$ $\displaystyle 117^{o}C$

Correct answer:

$28^{o}C$ $\displaystyle 28^{o}C$

Explanation:

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

Rearranging gives,

$Q=mC\bigtriangleup T$ $\displaystyle Q=mC\bigtriangleup T$

$Q=mC(T_{f}-T_{i})$ $\displaystyle Q=mC(T_{f}-T_{i})$

$423J=19g\times4.18\frac{J}{g^{o}C}\times(T_{f}-23^{o}C)$ $\displaystyle 423J=19g\times4.18\frac{J}{g^{o}C}\times(T_{f}-23^{o}C)$

$423J=79\frac{J}{^{o}C}\times(T_{f}-23^{o}C)$ $\displaystyle 423J=79\frac{J}{^{o}C}\times(T_{f}-23^{o}C)$

$\frac{423J}{79\frac{J}{^{o}C}}=T_{f}-23^{o}C$ $\displaystyle \frac{423J}{79\frac{J}{^{o}C}}=T_{f}-23^{o}C$

$5.35^{o}C=T_{f}-23^{o}C$ $\displaystyle 5.35^{o}C=T_{f}-23^{o}C$

$T_{f}=28^{o}C$ $\displaystyle T_{f}=28^{o}C$

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Example Question #41 : Physical Chemistry

A 20.5 g $\displaystyle 20.5 g$ metal at $37.1^{o}C$ $\displaystyle 37.1^{o}C$ was placed in 23.3 g $\displaystyle 23.3 g$ of water at $24.2^{o}C$ $\displaystyle 24.2^{o}C$ . The final temp of the water and metal was $26.0^{o}C$ $\displaystyle 26.0^{o}C$ . Assuming heat was not lost to the surroundings find the specific heat of the metal? The specific heat of water is $4.18\frac{J}{g^{o}C}$ $\displaystyle 4.18\frac{J}{g^{o}C}$ .

Possible Answers:

$0.897\frac{J}{g^{o}C}$ $\displaystyle 0.897\frac{J}{g^{o}C}$

$2.32\frac{J}{g^{o}C}$ $\displaystyle 2.32\frac{J}{g^{o}C}$

$1.2\frac{J}{g^{o}C}$ $\displaystyle 1.2\frac{J}{g^{o}C}$

$0.77\frac{J}{g^{o}C}$ $\displaystyle 0.77\frac{J}{g^{o}C}$

Correct answer:

$0.77\frac{J}{g^{o}C}$ $\displaystyle 0.77\frac{J}{g^{o}C}$

Explanation:

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

Heat is transferred from the metal to the water.

$-Q_{metal}=Q_{water}$ $\displaystyle -Q_{metal}=Q_{water}$

$-(mC\bigtriangleup T)=mC\bigtriangleup T$ $\displaystyle -(mC\bigtriangleup T)=mC\bigtriangleup T$

$-(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$ $\displaystyle -(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$

$-(20.5g\cdot C\cdot (26.0^{o}C-37.1^oC)=23.3g\cdot4.18\frac{J}{g^o}C(26.0^{o}C-24.2^{o}C)$ $\displaystyle -(20.5g\cdot C\cdot (26.0^{o}C-37.1^oC)=23.3g\cdot4.18\frac{J}{g^o}C(26.0^{o}C-24.2^{o}C)$

$-(-227.55g^{o}C\cdot C)=175.3092J$ $\displaystyle -(-227.55g^{o}C\cdot C)=175.3092J$

$227.55g^{o}C\cdot\ C=175.3092J$ $\displaystyle 227.55g^{o}C\cdot\ C=175.3092J$

$C=\frac{175.3092J}{227.55g^{o}C}=0.77\frac{J}{g^{o}C}$ $\displaystyle C=\frac{175.3092J}{227.55g^{o}C}=0.77\frac{J}{g^{o}C}$

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Example Question #361 : Gre Subject Test: Chemistry

What was the final temperature of the water if a 112 g $\displaystyle 112 g$ sample of water absorbs 231 J $\displaystyle 231 J$ of heat energy and heats up from $25.0^{o}C$ $\displaystyle 25.0^{o}C$ ? (specific heat of water= $4.18\frac{J}{g^{o}C}$ $\displaystyle 4.18\frac{J}{g^{o}C}$ )

Possible Answers:

$134^{o}C$ $\displaystyle 134^{o}C$

$25.5^{o}C$ $\displaystyle 25.5^{o}C$

$43.2^{o}C$ $\displaystyle 43.2^{o}C$

$75^{o}C$ $\displaystyle 75^{o}C$

Correct answer:

$25.5^{o}C$ $\displaystyle 25.5^{o}C$

Explanation:

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

Rearranging gives,

$Q=mC\bigtriangleup T$ $\displaystyle Q=mC\bigtriangleup T$

$Q=mC(T_{f}-T_{i})$ $\displaystyle Q=mC(T_{f}-T_{i})$

$231J=112g\times4.18\frac{J}{g^{o}C}\times(T_{f}-25.0^{o}C)$ $\displaystyle 231J=112g\times4.18\frac{J}{g^{o}C}\times(T_{f}-25.0^{o}C)$

$231J=468.16\frac{J}{^{o}C}\times(T_{f}-25.0^{o}C)$ $\displaystyle 231J=468.16\frac{J}{^{o}C}\times(T_{f}-25.0^{o}C)$

$\frac{231J}{468.16\frac{J}{^{o}C}}=T_{f}-25.0^{o}C$ $\displaystyle \frac{231J}{468.16\frac{J}{^{o}C}}=T_{f}-25.0^{o}C$

$0.493^{o}C=T_{f}-25.0^{o}C$ $\displaystyle 0.493^{o}C=T_{f}-25.0^{o}C$

$T_{f}=25.5^{o}C$ $\displaystyle T_{f}=25.5^{o}C$

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Example Question #1 : Heat And Temperature

A 10.2 g $\displaystyle 10.2 g$ metal at $72.9^{o}C$ $\displaystyle 72.9^{o}C$ was placed in 21.2 g $\displaystyle 21.2 g$ of water at $25.0^{o}C$ $\displaystyle 25.0^{o}C$ . The final temp of the water and metal was $53.3^{o}C$ $\displaystyle 53.3^{o}C$ . Assuming heat was not lost to the surroundings find the specific heat of the metal? The specific heat of water is $4.18\frac{J}{g^{o}C}$ $\displaystyle 4.18\frac{J}{g^{o}C}$ .

Possible Answers:

$465\frac{J}{g^{o}C}$ $\displaystyle 465\frac{J}{g^{o}C}$

$12.5\frac{J}{g^{o}C}$ $\displaystyle 12.5\frac{J}{g^{o}C}$

$2.6\frac{J}{g^{o}C}$ $\displaystyle 2.6\frac{J}{g^{o}C}$

$173\frac{J}{g^{o}C}$ $\displaystyle 173\frac{J}{g^{o}C}$

Correct answer:

$12.5\frac{J}{g^{o}C}$ $\displaystyle 12.5\frac{J}{g^{o}C}$

Explanation:

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

Heat is transferred from the metal to the water.

$-Q_{metal}=Q_{water}$ $\displaystyle -Q_{metal}=Q_{water}$

$-(mC\bigtriangleup T)=mC\bigtriangleup T$ $\displaystyle -(mC\bigtriangleup T)=mC\bigtriangleup T$

$-(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$ $\displaystyle -(mC(T_{f}-T_{i}))=-(mC(T_{f}-T_{i}))$

$-(10.2g\cdot C\cdot (53.3^{o}C-72.9^oC)=21.2g\cdot4.18\frac{J}{g^o}C(53.3^{o}C-25.0^{o}C)$ $\displaystyle -(10.2g\cdot C\cdot (53.3^{o}C-72.9^oC)=21.2g\cdot4.18\frac{J}{g^o}C(53.3^{o}C-25.0^{o}C)$

$-(-199.92g^{o}C\cdot C)=2507.83J$ $\displaystyle -(-199.92g^{o}C\cdot C)=2507.83J$

$199.92g^{o}C\cdot C=2507.83J$ $\displaystyle 199.92g^{o}C\cdot C=2507.83J$

$C=\frac{2507.83J}{199.92g^{o}C}=12.5\frac{J}{g^{o}C}$ $\displaystyle C=\frac{2507.83J}{199.92g^{o}C}=12.5\frac{J}{g^{o}C}$

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Example Question #361 : Gre Subject Test: Chemistry

How much heat is absorbed when 150 g $\displaystyle 150 g$ of water goes from $25.0^{o}C$ $\displaystyle 25.0^{o}C$ to $35.0^{o}C$ $\displaystyle 35.0^{o}C$ ? (Specific heat of water= $4.18 \frac{J}{g^{o}C}$ $\displaystyle 4.18 \frac{J}{g^{o}C}$ )

Possible Answers:

$2270\ J$ $\displaystyle 2270\ J$

$70\ J$ $\displaystyle 70\ J$

$6270\ J$ $\displaystyle 6270\ J$

$12\ J$ $\displaystyle 12\ J$

Correct answer:

$6270\ J$ $\displaystyle 6270\ J$

Explanation:

Specific heat is the amount of heat needed to raise 1 gram of a substance by 1oC. Calorimeters used for these types of experiments because they are designed to be well-insulated, so no heat is gained from or lost to the surroundings.

$C=\frac{Q}{m\times \bigtriangleup T}$ $\displaystyle C=\frac{Q}{m\times \bigtriangleup T}$

$Q=mC\bigtriangleup T$ $\displaystyle Q=mC\bigtriangleup T$

$Q=mC(T_{f}-T_{i})$ $\displaystyle Q=mC(T_{f}-T_{i})$

$Q=150g\cdot\ 4.18\frac{J}{g^{o}C}\cdot (35^{o}C-25^{o}C)$ $\displaystyle Q=150g\cdot\ 4.18\frac{J}{g^{o}C}\cdot (35^{o}C-25^{o}C)$

$Q=6270\ J$ $\displaystyle Q=6270\ J$

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GRE Subject Test: Chemistry : Heat and Temperature

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