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Alexus [3.1K]
3 years ago
9

Period, block, and group

Chemistry
1 answer:
Sedaia [141]3 years ago
8 0

Answer:

what do you mean

Explanation:

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A 76.0-gram piece of metal at 96.0 °C is placed in 120.0 g of water in a calorimeter at 24.5 °C. The final temperature in the ca
Phoenix [80]

The specific heat capacity of the metal given the data from the question is 0.66 J/gºC

<h3>Data obtained from the question</h3>
  • Mass of metal (M) = 76 g
  • Temperature of metal (T) = 96 °C
  • Mass of water (Mᵥᵥ) = 120 g
  • Temperature of water (Tᵥᵥ) = 24.5 °C
  • Equilibrium temperature (Tₑ) = 31 °C
  • Specific heat capacity of the water (Cᵥᵥ) = 4.184 J/gºC
  • Specific heat capacity of metal (C) =?

<h3>How to determine the specific heat capacity of the metal</h3>

The specific heat capacity of the sample of the metal can be obtained as follow:

Heat loss = Heat gain

MC(M –Tₑ) = MᵥᵥCᵥᵥ(Tₑ – Tᵥᵥ)

76 × C × (96 – 31) = 120 × 4.184 × (31 – 24.5)

C × 4940 = 3263.52

Divide both side by 4940

C = 3263.52 / 4940

C = 0.66 J/gºC

Learn more about heat transfer:

brainly.com/question/6363778

#SPJ1

6 0
2 years ago
The density of ethanol, a colorless liquid that is commonly known as grain alcohol, is 0.798 g/mL Calculate the mass of 205 mL o
katovenus [111]

Answer:

Mass of 205 mL of the liquid is 164 g

Explanation:

We know, density=\frac{mass}{volume}

Here density of liquid is 0.798 g/mL and volume of liquid is 205 mL

So, mass of liquid = density\times volume

                              = (0.798 g/mL)\times (205 mL)

                              = 164 g

hence mass of 205 mL of the liquid is 164 g.

8 0
3 years ago
How much heat will be released if 9.75 g of aluminum reacts with excess ammonium nitrate (NH₄NO₃) according to the following equ
Mandarinka [93]

Not enough info

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7 0
3 years ago
When a 1.00-g sample of methane gas was burned with excess oxygen in the calorimeter, the temperature increased by 7.3°C. When
Advocard [28]

Answer:

The energies of  combustion (per gram) for hydrogen and methane are as follows: Methane = 82.5 kJ/g;  Hydrogen = 162 kJ/g

<em>Note: The question is incomplete. The complete question is given below:</em>

To compare the energies of combustion of these fuels, the  following experiment was carried out using a bomb  calorimeter with a heat capacity of 11.3 kJ/℃.  When a 1.00-g sample of methane gas burned with

<em>excess oxygen in the calorimeter, the temperature  increased by 7.3℃. When a 1.00 g sample of  hydrogen gas was burned with excess oxygen, the temperature increase was 14.3°C. Compare the energies of  combustion (per gram) for hydrogen and methane.</em>

Explanation:

From the equation of the first law of thermodynamics, ΔU = Q + W

Since there is no expansion work in the bomb calorimeter,  ΔU = Q

But Q = CΔT

where C is heat capacity of the bomb calorimeter =  11.3
kJ/ºC; ΔT = temperature change

For combustion of methane gas:

Q per gram = (
11.3
kJ/ºC * 7.3°C)/1.0g

Q = 83 kJ/g

For combustion of hydrogen gas:

Q per gram = (
11.3
kJ/ºC * 14.3°C)/1.0g

Q = 162 kJ/g

3 0
3 years ago
Give an example of at least one element made up of molecules and one compound made up of molecules.
zavuch27 [327]
I think mercury for element and sodium hypochlorite
8 0
3 years ago
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