What is the average thermal energy of ice?

If 56 J of heat is added to an aluminum can with a mass of 23.6 g , what is its temperature change? Specific heat capacity of al

elena-s [515]

Answer:

2.627775588 degrees Celsius (with 2 sig figs)

Explanation:

We need to use our equation q=m×s×(change in temp) and solve for our change in temperature. So divide both sides by m×s and you'll get:

Change in temp=q/(m×s) Where q= J of heat m=mass and s= specific heat

So now we just plug our numbers in:

56J/(23.6g×0.903J/g°C)= 2.627775588 and since 56 only has 2 sig figs, we round the final answer to 2.6°C

3 0

3 years ago

bartleby whihch of the foololwing is the correct cell notation for the reaction Hg2 Cd(s)-> Cd2 2Hg(l)

Misha Larkins [42]

Cd2+ + 2Hg Cd + Hg22+. Both Cd2+ + 2e Cd(s) -0.40 and Hg22+ + 2e 2Hg(l) 0.79

A chemical reaction known as an oxidation-reduction (redox) reaction includes the exchange of electrons between two substances.

Any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by acquiring or losing an electron is referred to as an oxidation-reduction reaction. Decomposition Reaction is one of the several redox reactions.

This is the redox reaction's overall cell potential. Cd2+ + 2Hg Cd + Hg22+. Both Cd2+ + 2e Cd(s) -0.40 and Hg22+ + 2e 2Hg(l) 0.79

Reduction describes the increase in electrons. Oxidation and reduction always occur jointly because any loss of electrons by one substance must be followed by a gain of electrons by another.

Therefore, oxidation-reduction processes or simply redox reactions are other names for electron-transfer events.

Learn more about redox reactions here brainly.com/question/8727728.

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3 0

2 years ago

A voltaic cell is based on the reduction of ag (aq) to ag(s) and the oxidation of sn(s) to sn2 (aq).

Annette [7]

Half-reaction for the cell's anode is given below:

Anode : $\\Sn(s) \rightarrow Sn^{2+} (aq) +2e^{-}$

The anode is defined as the electrode at which electrons leave the cell and oxidation occurs, and the cathode as the electrode at which electrons enter the cell and reduction occurs. The anode is usually the positive side.

Learn more about anode here:

brainly.com/question/4052514

Your given question is quite incomplete here is complete question.

A voltaic cell is based on the reduction of _ Agt(aq) to Ag(s) and the oxidation of Sn(s) to Sn2+(aql) : Part 1 Include the phases of all species in the chemical equation: (aqh Anode: Sn(s) Sn?+ (aq)

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4 0

2 years ago

The density of silver is 10.5 g/cm3. What is the mass (in kilograms) of a cube of silver that measures 0.94 m on each side?

Rzqust [24]

Answer:

8721.132 Kg.

Explanation:

The following data were obtained from the question:

Density (D) of silver = 10.5 g/cm³

Length (L) of silver = 0.94 m

Mass (m) of silver =.?

Next, we shall determine the volume of silver. This can be obtained as follow:

Volume = Length × Length × Length

Volume = L × L × L

Volume = L³

Length (L) of silver = 0.94 m

Volume (V) of silver =?

Volume (V) of silver = 0.94³

Volume (V) of silver = 0.830584 m³

Next, we shall convert 0.830584 m³ to cm³. This can be obtained as follow:

1 m³ = 1×10⁶ cm³

Therefore,

0.830584 m³ = 0.830584 m³ / 1 m³ × 1×10⁶ cm³

0.830584 m³ = 830584 cm³

Therefore, 0.830584 m³ is equivalent 830584 cm³.

Thus, the volume of the silver is 830584 cm³.

Next, we shall determine the mass of the silver. This can be obtained as follow:

Density (D) of silver = 10.5 g/cm³

Volume of the silver = 830584 cm³.

Mass of silver =.?

Density = mass /

10.5 = mass of silver /830584

Cross multiply

Mass of silver = 10.5 × 830584

Mass of silver = 8721132 g

Finally, we shall convert the mass of silver, 8721132 g to kilogram (kg). This can be obtained as follow:

1000 g = 1 Kg

Therefore,

8721132 g = 8721132 g / 1000 g × 1 Kg

8721132 g = 8721.132 Kg

Therefore, the mass of each cube of silver is 8721.132 Kg

3 0

3 years ago

Now they feel it is best to have you identify an unknown gas based on its properties. Suppose 0.508 g of a gas occupies a volume

pishuonlain [190]

Answer: Option (b) is the correct answer.

Explanation:

The given data is as follows.

mass = 0.508 g, Volume = 0.175 L

Temperature = (25 + 273) K = 298 K, P = 1 atm

As per the ideal gas law, PV = nRT.

where, n = no. of moles = $\frac{mass}{\text{molar mass}}$

Hence, putting all the given values into the ideal gas equation as follows.

PV = $\frac{mass}{\text{molar mass}} \times RT$

1 atm \times 0.175 L = $\frac{0.508 g}{\text{molar mass}} \times 0.0821 L atm/ K mol \times 298 K$

= 71.02 g

As the molar mass of a chlorine atom is 35.4 g/mol and it exists as a gas. So, molar mass of $Cl_{2}$ is 70.8 g/mol or 71 g/mol (approx).

Thus, we can conclude that the gas is most likely chlorine.

4 0

3 years ago