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3 years ago

What does the symbol Cp

Chemistry

1 answer:

xenn [34]3 years ago

8 0

Answer:

From what i've learned so far, the correct answer is "Heat at a constant Pressure" or "Specific Heat"

Explanation:

Hope this helps!

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Convert 53.4 g to ounces

MrMuchimi

The answer is 1.884 ounce.

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3 years ago

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Identify the mole ratio that can be derived from the following balanced chemical reaction: 4 Fe + 3 O2 --> 2 Fe2O3 a. 4 mol F

Arlecino [84]

To determine the mole ratio between two substances, all you need to do is look at the balanced equation for the coefficients in front of the substances you are interested in.

Answer: A

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4 years ago

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Most chemical reactions release energy or are exothermic. However, some reactions, such as some decompositions, absorb energy. T

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Answer:

C) The products have more energy stored in their chemical bonds.

Explanation:

In such reactions that absorb energy, the products have more energy stored in their chemical bonds.

For endothermic changes, heat is absorbed from the surrounding hence the surrounding becomes colder at the end of the changes.

The heat energy level of the products is higher than that of the reactants.

Exothermic reactions releases heat to the surroundings. The sum of heat contents of the products is less than that of the hat contents of the reactants.
Examples of such processes are burning and dissolution.

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3 years ago

Use the drop-down menus to match the type of intermolecular force to its name.

geniusboy [140]

Answer:

Dipole-dipole interactions : occur between polar molecules

Dipole-induced dipole interactions: occur between polar and nonpolar molecules

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van der Waals forces: electrostatic interactions between partially charged regions of a molecule

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3 years ago

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10.0 g Cu, C Cu = 0.385 J/g°C 10.0 g Al, C Al = 0.903 J/g°C 10.0 g ethanol, Methanol = 2.42 J/g°C 10.0 g H2O, CH2O = 4.18 J/g°C

Mazyrski [523]

Answer:

Lead shows the greatest temperature change upon absorbing 100.0 J of heat.

Explanation:

$Q=mc\Delte T$

Q = Energy gained or lost by the substance

m = mass of the substance

c = specific heat of the substance

ΔT = change in temperature

1) 10.0 g of copper

Q = 100.0 J (positive means that heat is gained)

m = 10.0 g

Specific heat of the copper = c = 0.385 J/g°C

$\Delta T=\frac{Q}{mc}$

$=\frac{100.0 J}{10 g\times 0.385J/g^oC}=25.97^oC$

2) 10.0 g of aluminium

Q = 100.0 J (positive means that heat is gained)

m = 10.0 g

Specific heat of the aluminium= c = 0.903 J/g°C

$\Delta T=\frac{Q}{mc}$

$=\frac{100.0 J}{10 g\times 0.903 J/g^oC}=11.07^oC$

3) 10.0 g of ethanol

Q = 100.0 J (positive means that heat is gained)

m = 10.0 g

Specific heat of the ethanol= c = 2.42 J/g°C

$\Delta T=\frac{Q}{mc}$

$=\frac{100.0 J}{10 g\times 2.42 J/g^oC}=4.13 ^oC$

4) 10.0 g of water

Q = 100.0 J (positive means that heat is gained)

m = 10.0 g

Specific heat of the water = c = 4.18J/g°C

$\Delta T=\frac{Q}{mc}$

$=\frac{100.0 J}{10 g\times 4.18 J/g^oC}=2.39 ^oC$

5) 10.0 g of lead

Q = 100.0 J (positive means that heat is gained)

m = 10.0 g

Specific heat of the lead= c = 0.128 J/g°C

$\Delta T=\frac{Q}{mc}$

$=\frac{100.0 J}{10 g\times 0.128 J/g^oC}=78.125^oC$

Lead shows the greatest temperature change upon absorbing 100.0 J of heat.

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4 years ago