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3 years ago

How many joules of energy are required to melt 423g of water at 0°C?

Chemistry

2 answers:

Mkey [24]3 years ago

6 0

The amount of heat needed to melt 423 g of water at 0°C is 141282 J

The heat required to melt water can be obtained by using the following formula:

Q is the heat required.

L is the latent heat of fusion (334 J/g)

m is the mass.

With the above formula, we can obtain the heat required to melt the water as illustrated below:

Mass of water (m) = 423 g

Latent heat of fusion (L) = 334 J/g

<h3>Heat (Q) required =? </h3>

Q = mL

Q = 423 × 334

Therefore, the amount of heat needed to melt 423 g of water at 0°C is 141282 J

Learn more: brainly.com/question/17084080

Julli [10]3 years ago

5 0

Answer: hope this helps mark me BRAINLEST plz ;)

Explanation:42. Practice Problem  How many joules of energy are required to vaporize 423g of water at 100oC and 1atmosphere of pressure. q = mHv m = 423 g Hv = 2260 J/gq = (423g) (2260J/g) = 955,980 J = 956 43. Table T – Heat Formulas

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Pb(CH3COO)2 + H2S --> PbS + CH3COOH 1. How many moles are produced of PbS when 5.00 grams of Pb(CH3COO)2 is reacted with H2S?

shutvik [7]

Answer:

1. 0.0154mole of PbS

2. Double displacement reaction

Explanation:

First, let write a balanced equation for the reaction. This is illustrated below:

Pb(CH3COO)2 + H2S —> PbS + 2 CH3COOH

Molar Mass of Pb(CH3COO)2 = 207 + 2(12 + 3 + 12 + 16 +16) = 207 + 2(59) = 207 + 118 = 325g

Mass of Pb(CH3COO)2 = 5g

Number of mole = Mass /Molar Mass

Number of mole of Pb(CH3COO)2 = 5/325 = 0.0154mole

From the equation,

1mole of Pb(CH3COO)2 produced 1mole of PbS.

Therefore, 0.0154mole of Pb(CH3COO)2 will also produce 0.0154mole of PbS

2. The name of the reaction is double displacement reaction since the ions in the two reactants interchange to form two different products

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Calcular la normalidad de 1 Kg de sulfuro de aluminio en 5000 ml de solucion.

Troyanec [42]

Calculate the normality of 1 Kg of aluminum sulfide in 5000 ml of solution.

Normality comes out to be 8.11

<h3> Given </h3>

Mass of solute: 1000g
Volume of solution (V): 5000 ml = 5 liters
Equivalent mass of solute (E) = molar mass / n-factor

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So, on calculating equivalent mass is equal to 24.66g

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N= $\frac{1000}{24.66*5}$

Therefore, normality of 1 kg aluminum sulfide is 8.11

Learn more about normality here brainly.com/question/25507216

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2 years ago

How many moles of sulfur will be needed to oxidize 3 moles of zinc to zinc sulfide

Ksenya-84 [330]

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Solution : Given,

Moles of zinc = 3 moles

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From the balanced reaction, we conclude that

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3 years ago