If you combine 400.0 mL of water at 25.00 �C and 140.0 mL of water at...

If you combine 400.0 mL of water at 25.00 �C and 140.0 mL of water at 95.00 �C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

Expert Solution

Let the final temperature of the mixture be t^oC ( Obviously, 95.00 ^oC > t ^oC > 25.00 ^oC )

Mass of the sample of cold water = ( Volume x Density ) = ( 400 mL x 1.00 g/mL ) = 400 g

Specific heat capacity of water = 4.184 J/g. ^oC

Heat gained by cold water = Mass x Specific heat capacity of water x Change in temperature

= (400g ) x ( 4.184 J/g. ^oC ) x ( t - 25) ^oC

Mass of the sample of hot water = ( 140 mL x 1.00 g/mL) = 140 g

Heat lost by hot water = ( 140 g) x ( 4.184 J/g. ^oC) x ( 95 - t) ^oC

According to the principle of calorimetry,

Heat gained = Heat lost

(400 g) x ( 4.184 J/g. ^oC) x ( t - 25) ^oC = (140 g) x ( 4.184 J/g. ^oC) x ( 95 - t ) ^oC

400 ( t - 25 ) = 140 ( 95 - t)

400 t - 10000 = 13300 - 140t

540t = 23300

t = 43.15

Therefore, the final temperature of the mixture is 43.15 ^oC.

queen_honey_blossom answered 2 years ago

If you combine 280.0 mL of water at 25.00 °C and 140.0 mL of water at...

If you combine 280.0 mL of water at 25.00 °C and 140.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

If you combine 360.0 mL of water at 25.00 °C and 100.0 mL of water at...

If you combine 360.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

If you combine 330.0 mL of water at 25.00 °C and 100.0 mL of water at...

If you combine 330.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

f you combine 320.0 mL of water at 25.00 °C and 100.0 mL of water at...

f you combine 320.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

You mix a 140.0 −mL−mL sample of a solution that is 0.0124 MM in NiCl2NiCl2 with...

You mix a 140.0 −mL−mL sample of a solution that is 0.0124 MM in NiCl2NiCl2 with a 200.0 −mL−mL sample of a solution that is 0.350 MM in NH3NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq)Ni2+(aq) remains? The value of KfKf for Ni(NH3)62+Ni(NH3)62+ is 2.0×1082.0×108. Express the concentration to two significant figures and include the appropriate units.

When 20.0g of steam at 140.0 °C condenses into 200.0g liquid water at 25.0 °C, what...

When 20.0g of steam at 140.0 °C condenses into 200.0g liquid water at 25.0 °C, what will be the final temperature of the water? Assume that everything takes place in a perfectly insulated enclosure from which there is no heat leak. Data: heat of vaporization for water (Hvap): 40.7 kJ/mole Heat capacity of steam: 2.09 J/g-°C Heat capacity of water: 4.184 J/g-°C Please Explain Step by step

Pipette 25.00 mL of the prepared sample into a 250 mL conical flask and add 20 mL of water.

Assay for Al3+ Pipette 25.00 mL of the prepared sample into a 250 mL conical flask and add 20 mL of water. Then, with swirling add, by pipette, 25.00 mL of 0.01 mol L-1 EDTA (you need to copy down the EXACT concentration (it therefore should not have just one or two significant figures!) of EDTA provided). Continue stirring, and add 20 mL of pH 4.5 buffer. (NOTE: The order of these additions is important). Heat the solution in...

1.50 mL of 0.15M Fe2(SO4)3 is diluted with deionized water to 25.00 mL in a volumetric...

1.50 mL of 0.15M Fe2(SO4)3 is diluted with deionized water to 25.00 mL in a volumetric flask. What is the concentration (in both molarity and μg/mL) of iron (not†Fe2(SO4)3) in the diluted sample?

Calculate the pH after addition of a) 0.00 mL b) 25.00 mL c) 50.00 mL d)...

Calculate the pH after addition of a) 0.00 mL b) 25.00 mL c) 50.00 mL d) 60.00 mL of 0.1000 M HCl in the titration of 50.00 mL of 0.1000 M hydrazine. Ka(N2H5+)=1.05×10−8. Please show all steps thank you!

You place 59.7 ml of 0.605 M NaOH in a coffee- cup calorimeter at 25.00°C and...

You place 59.7 ml of 0.605 M NaOH in a coffee- cup calorimeter at 25.00°C and add 76 ml of 0.605 M HCl, also at 25.00°C. After stirring, the final temperature is 27.84°C. [Assume the total volume is the sum of the individual volumes and that the final solution has the same density (1.00 g/ml) and specific heat capacity (4.184 J/gK)]. Calculate the change in enthalpy of the reaction in kJ/mol of water formed. Enter to 1 decimal place. Hint:...

Question