Question

If you combine 330.0 mL of water at 25.00 °C and 130.0 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.

Answer #1

If you combine 360.0 mL of water at 25.00 °C and 130.0 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 430.0 mL of water at 25.00 °C and 130.0 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 440.0 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 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.
Answer: _____celsius

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 a system has 4.50 × 102 kcal of work done to it, and releases
5.00 × 102 kJ of heat into its surroundings, what is the change in
internal energy of the system?

If you combine 360.0mL of water at 25.00C and 110.0mL of water
at 95.00C, what is the final temperature of the mixture? Use 1.00
g/mL as the density of water. Answer in Celcius.

If you have 410.0 g of water at 25.00 °C in an insulated vessel
and add 120.0 g of water at 95.00 °C, what is the final temperature
of the mixture?

You place 40.3 ml of 0.366 M NaOH in a coffee- cup calorimeter
at 25.00°C and add 64.8 ml of 0.366 M HCl, also at 25.00°C. After
stirring, the final temperature is 27.93°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 (ΔH) of
the reaction in kJ/mol of water formed. Enter to 1 decimal place....

When you combine 50.0 mL of 0.100 M silver nitrate with 50.0 mL
of 0.100 M HCl, the temperature changes from 23.40˚C to 24.21˚C.
Calculate
ΔHrxn.
(Assume a specific heat of 4.184 J / g · ˚C and use 1.00 g/mL as
the density.)

In a coffee-cup calorimeter, 130.0 mL of 1.0 M NaOH and 130.0 mL
of 1.0 M HCl are mixed. Both solutions were originally at 26.8°C.
After the reaction, the final temperature is 33.5°C. Assuming that
all the solutions have a density of 1.0 g/cm and a specific heat
capacity of 4.18 J/°C ⋅ g, calculate the enthalpy change for the
neutralization of HCl by NaOH. Assume that no heat is lost to the
surroundings or to the calorimeter.
Enthalpy change...

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