Question

1) A 32 g stainless steel ball at 110.5°C is placed in a constant pressure calorimeter...

1) A 32 g stainless steel ball at 110.5°C is placed in a constant pressure calorimeter containing 100 ml of water at 20 °C. Calculate the final temperature of water. The specific heat of the ball is 0.474 J/g°C and the specific heat of water is 4.18 J/g°C.

explain plz

Homework Answers

Answer #1

Let us denote water by symbol 1 and ball by symbol 2

since volume of water is 100 mL and density is 1 g/mL,mass of water = 100 g

m1 = 100 g

T1 = 20 oC

C1 = 4.18 J/goC

m2 = 32 g

T2 = 110.5 oC

C2 = 0.474 J/goC

Let the final temperature be T oC

we have below equation to be used:

heat lost by 2 = heat gained by 1

m2*C2*(T2-T) = m1*C1*(T-T1)

32.0*0.474*(110.5-T) = 100.0*4.18*(T-20.0)

15.168*(110.5-T) = 418*(T-20.0)

1676.064 - 15.168*T = 418*T - 8360

T= 23.2 oC

Answer: 23.2 oC

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
3.00 g of potassium hydroxide (KOH) pellets are put into a constant-pressure calorimeter containing 250 mL...
3.00 g of potassium hydroxide (KOH) pellets are put into a constant-pressure calorimeter containing 250 mL of water. The initial temperature of the water is 22.3°C. The mixture is then stirred until all of the KOH is dissolved. The final temperature of the solution is measured and recorded as 29.7°C. Calculate the heat of solution for potassium hydroxide (ΔHsoln). The specific heat capacity of the solution may be assumed to be the same as that of water since this is...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 60.93 grams of gold to 98.87 °C and then drops it into a cup containing 79.68 grams of water at 24.46 °C. She measures the final temperature to be 26.11 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling...
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine...
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A chunk of zinc weighing 18.01 grams and originally at 98.77 °C is dropped into an insulated cup containing 83.17 grams of water at 20.02 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.56...
300.0 g of copper is heated to 100.0*C and transferred quickly to a calorimeter containing 400.0...
300.0 g of copper is heated to 100.0*C and transferred quickly to a calorimeter containing 400.0 grams of water initially at 25.0*C. If the final temperature is 29.4*C, calculate the specific heat of copper. The specific heat of water is 4.18 J/g-*C. What assumptions must be made about the calorimeter? How is the first law of thermodynamics and law of conservation of energy used in this experiment.
1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water...
1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 27.0°C. - How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.) - What is the specific heat (in J/g·°C) of the metal? 2. A 0.529 g sample of KCl is added...
two parts for one question ----------------------------------------- In the laboratory a "coffee cup" calorimeter, or constant pressure...
two parts for one question ----------------------------------------- In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is...
When a 290-g piece of iron at 170 ∘C is placed in a 95-gg aluminum calorimeter...
When a 290-g piece of iron at 170 ∘C is placed in a 95-gg aluminum calorimeter cup containing 250 g of liquid at 10∘C, the final temperature is observed to be 32 ∘C. The value of specific heat for iron is 450 J/kg⋅C∘, and for aluminum is 900 J/kg⋅C∘ Part A Determine the specific heat of the liquid. Express your answer using two significant figures.
A lead (Pb) pellet having a mass of 26.47 g at 89.98°C was placed in a...
A lead (Pb) pellet having a mass of 26.47 g at 89.98°C was placed in a constant-pressure calorimeter of negligible heat capacity containing 100.0 mL of water. The water temperature rose from 22.50°C to 23.17°C. What is the specific heat of the lead pellet?