Question

A 2.74g sample of a substance assumed to be pure gold is warmed to 80.0C and...

A 2.74g sample of a substance assumed to be pure gold is warmed to 80.0C and submerged in to 15.2 g of water, initially at 24.7 C. The final temperature of the mixture is 25.30C. What is the heat capacity of the substance? could this substance be pure gold?

Homework Answers

Answer #1

m(water) = 15.2 g

T(water) = 24.7 oC

C(water) = 4.184 J/goC

m(gold) = 2.74 g

T(gold) = 80.0 oC

C(gold) = to be calculated

We will be using heat conservation equation

use:

heat lost by gold = heat gained by water

m(gold)*C(gold)*(T(gold)-T) = m(water)*C(water)*(T-T(water))

2.74*C(gold)*(80.0-25.3) = 15.2*4.184*(25.3-24.7)

149.878*C(gold) = 38.1581

C(gold)= 0.255 J/goC

Answer: 0.255 J/goC

Actual specific heat capacity of gold is 0.129 J/goC

So, this can’t be pure gold

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
A 2.44 g sample of a substance suspected of being pure gold is warmed to 72.5...
A 2.44 g sample of a substance suspected of being pure gold is warmed to 72.5 ∘C and submerged into 15.0 g of water initially at 24.8 ∘C. The final temperature of the mixture is 26.4 ∘C. What is the heat capacity of the unknown substance?Express your answer using two significant figures. Could the substance be pure gold?
A 31.7 g wafer of pure gold initially at 69.7 ∘C is submerged into 64.1 g...
A 31.7 g wafer of pure gold initially at 69.7 ∘C is submerged into 64.1 g of water at 27.4 ∘C in an insulated container. What is the final temperature of both substances at thermal equilibrium?
A 31.5 g wafer of pure gold initially at 69.8 ∘C is submerged into 64.1 g...
A 31.5 g wafer of pure gold initially at 69.8 ∘C is submerged into 64.1 g of water at 27.6 ∘C in an insulated container. What is the final temperature of both substances at thermal equilibrium?
A 31.1g wafer of pure gold initially at 69.4 degrees C is submerged into 63.2g of...
A 31.1g wafer of pure gold initially at 69.4 degrees C is submerged into 63.2g of water at 27.1 degrees C in an insulated container. What is the final temperature of both substances at thermal equilibrium?
A 25 g gold nugget with an initial temperature of 60 °C is dropped into an...
A 25 g gold nugget with an initial temperature of 60 °C is dropped into an insulated cup containing 100 ml of water initially at a temperature of 5°C. What is the final temperature after thermal equilibrium is established? Table 3.4 Specific Heat Capacities of Some Common Substances Substance Specific Heat Capacity (J/g °C) Lead 0.128 Gold 0.128 Silver 0.235 Copper 0.385 Iron 0.449 Aluminum 0.903 Ethanol 2.42 Water 4.184
A student heats up a 2.5-g gold block (cs = 0.13 J/g-K) from 13.5 oC to...
A student heats up a 2.5-g gold block (cs = 0.13 J/g-K) from 13.5 oC to 22.8 oC. a. What is the heat capacity of this gold block? b. What is the molar heat capacity of gold? c. How many joules are required to heat this gold block from 13.5 oC to 22.8 oC? d. If this gold block is submerged into 50 mL of water (cs = 4.18 J/g°-K) at 50 oC after it reaches 22.8 oC, indicate the...
A 27.0 −g aluminum block is warmed to 65.6 ∘C and plunged into an insulated beaker...
A 27.0 −g aluminum block is warmed to 65.6 ∘C and plunged into an insulated beaker containing 55.1 g water initially at 22.4 ∘C. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?
A    1.6-g sample of a metal that has the appearance of gold requires 5.8J of...
A    1.6-g sample of a metal that has the appearance of gold requires 5.8J of energy to change it’s temperature from 23C to 41 C. Is the metal pure gold? B   If 294J of heat is transferred to a 10.0 g sample of silver at 25⁰C, what is the final temperature of the silver?
A 26.5-g aluminum block is warmed to 65.2 ∘Cand plunged into an insulated beaker containing 55.2...
A 26.5-g aluminum block is warmed to 65.2 ∘Cand plunged into an insulated beaker containing 55.2 g of water initially at 22.2 ∘C. The aluminum and the water are allowed to come to thermal equilibrium. (Cs,H2O=4.18 J/g⋅∘C, Cs,Al=0.903J/g⋅∘C)​ Assuming that no heat is lost, what is the final temperature of the water and aluminum?​
A 53.25 g sample of a substance is initially at 28.3 °C. After absorbing 2927 J...
A 53.25 g sample of a substance is initially at 28.3 °C. After absorbing 2927 J of heat, the temperature of the substance is 115.8 °C. What is the specific heat (c) of the substance?