Question

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?

Answer #1

**a)
m1 = V1*density
=280 mL * 1 g/mL
= 280 g
T1 = 25 oC**

**m2 = V2*density
=140 mL * 1 g/mL
= 140 g
T2 = 95 oC**

**Let final temperature be ToC
use:
Heat lost by m2 = heat gained by m1
m2*C*(95-T) = m1*C*(T-25)
140*(95-T) = 280*(T-25)
13300 - 140*T = 280*T - 7000
T = 48.33 oC
Answer: 48.33 oC**

**2)
Q = -5.00 *10^2 KJ
W = 4.50*10^2 KCal
= 4.5*10^2 * 4.184 KJ
= 1.88*10^3 KJ**

**delta U = Q + W
= (-5.00 *10^2) + (1.88*10^3)
= 1.38*10^3 KJ
Answer: 1.38*10^3 KJ**

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 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 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 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.

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 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.

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....

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?

A 275 g sample of nickel at 100.0ºC is placed in 100.0 mL of
water at 22.0ºC. What is the final temperature of the mixture,
assuming no heat is lost to the surroundings? The specific heat
capacity of Ni is 0.444 J/(g.ºC). The density of water is 1.00 g/mL
and the specific heat capacity of water is 4.18 J/(g.ºC.

Part A A calorimeter contains 21.0 mL of water at 11.0 ∘C . When
1.60 g of X (a substance with a molar mass of 72.0 g/mol ) is
added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the
temperature of the solution increases to 26.0 ∘C . Calculate the
enthalpy change, ΔH, for this reaction per mole of X. Assume that
the specific heat of the resulting solution is equal to that of
water [4.18 J/(g⋅∘C)], that density of water...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 7 minutes ago

asked 27 minutes ago

asked 33 minutes ago

asked 36 minutes ago

asked 52 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 3 hours ago

asked 4 hours ago

asked 4 hours ago