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3 years ago

Determine the amount of heat (in kj) required to vaporize 1.55 kg of water at its boiling point. for water, δhvap

1 answer:

5 0

Heat required to vaporize 1 mol of water from water at 100C to steam at 100C = 40.7 kJ
1 mol of water weighs = 18.015g
1.55 kg = 1550/18.015 mol = 86.03 mol

Heat required to vaporize :
= 86.03 mol x 40.7 kJ

= 3501.421 kJ

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Boiling Point is the __________. *

sergiy2304 [10]

Boiling point is the temperature at which a liquid boils and turns to a gas.

Hope this helps!! (:

7 0

2 years ago

Carbon dioxide in the atmosphere dissolves in raindrops to produce carbonic acid (H2CO3), causing the pH of clean, unpolluted ra

anastassius [24]

Answer:

The range of [H⁺] is from 2.51 x 10⁻⁶ M to 6.31 x 10⁻⁶ M,

Explanation:

To answer this problem we need to keep in mind the definition of pH:

pH = -log [H⁺]

So now we calculate [H⁺] using a pH value of 5.2 and of 5.6:

5.2 = -log [H⁺]

-5.2 = log [H⁺]

$10^{-5.2}$ = [H⁺]

6.31 x 10⁻⁶ M = [H⁺]

5.6 = -log [H⁺]

-5.6 = log [H⁺]

$10^{-5.6}$ = [H⁺]

2.51 x 10⁻⁶ M = [H⁺]

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3 years ago

Identify the catalyst in this reaction, explain how

telo118 [61]

Question:

Sulfuric acid was once produced through the reaction of sulfur trioxide with water. Sulfur trioxide can form through the reaction of sulfur dioxide and oxygen gas. When nitrogen monoxide gas is added to the system, the reaction speeds up significantly because it proceeds through the following steps:

equations

Identify the catalyst in this reaction, explain how you know it is the catalyst, and describe how it increases the rate of the reaction.

Answer:

It is present but not consumed

NO Lowers the activation energy of the reaction

Explanation:

A catalyst is a substance that is present in a chemical reaction and enables the reaction to occur at a faster rte but does not take part n the reaction

Therefore, whereby NO is not consumed, it is the catalyst

It functions by lowering the activation energy

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3 years ago

Three kilograms of steam is contained in a horizontal, frictionless piston and the cylinder is heated at a constant pressure of

lakkis [162]

Answer:

Final temperature: 659.8ºC

Expansion work: 3*75=225 kJ

Internal energy change: 275 kJ

Explanation:

First, considering both initial and final states, write the energy balance:

$U_{2}-U_{1}=Q-W$

Q is the only variable known. To determine the work, it is possible to consider the reversible process; the work done on a expansion reversible process may be calculated as:

$dw=Pdv$