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3 years ago

How much heat in joules and in calories is required to heat at 28.4g( 1 oz) ice cube from -23C TO 1.0C

1 answer:

3 0

1426.58 J and 340.90 calories heat in joules and in calories is required to heat at 28.4g( 1 oz) ice cube from -23C TO 1.0C.

Explanation:

Data given:

mass = 28.4 gram

initial temperature = -23 degrees

final temperature = 1degress

change in temperature ΔT = Tfinal - Tinitial

ΔT = 1 -(-23)

ΔT = 24 degrees

specific heat capacity of ice cube c = 2.093 J/g C

Formula used:

q = mc ΔT

putting the values in the equation:

q= 28.4 x 2.093 x 24

= 1426.58 J

ENERGY IN CALORIES:

340.90 calories is the energy is required in the process.

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1 year ago

a glass of ice at 0 degrees Celsius changes to a glass of water at 0 degrees Celsius what caused the ice to change to water

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3 years ago

What is the IMA of the lever pictured?<br><br><br><br> 0.18<br> 0.20<br> 0.90<br> 5

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3 years ago

The atomic mass of Cu is 63.5. Find its electrochemical equivalent

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Answer:

The electrochemical equivalent of copper, Cu, is 3.29015544 × 10⁻⁷ g/C

Explanation:

The given parameters are;

The element for which the electrochemical equivalent is sought = Copper

The atomic mass of copper = 63.5

The electrochemical equivalent, 'Z', of an element or a substance is the mass, 'm', of the element or substance deposited by one coulomb of electricity, which is equivalent to a 1 ampere current flowing for a period of 1 second

Mathematically, we have;

m = Z·I·t = Z·Q

We have;

Cu²⁺ (aq) + 2·e⁻ → Cu

Therefore, one mole of Cu, is deposited by 2 moles of electrons

The charge carried one mole of electrons = 1 Faraday = 96500 C

∴ The charge carried two moles of electrons, Q = 2 × 96500 C = 193,000 C

Given that the mass of an atom of Cu = 63.5 a.m.u., the mass of one mole of Cu, m = 63.5 g

$Z = \dfrac{m}{Q} = \dfrac{63.5 \ g}{193,000 \ C} = 3.29015544 \times 10^{-4} \, g \cdot C^{-1}$

∴ Z = 3.29015544 × 10⁻⁴ g/C = 3.29015544 × 10⁻⁷ g/C

The electrochemical equivalent of copper, Cu, is Z = 3.29015544 × 10⁻⁷ g/C

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3 years ago