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hammer [34]
3 years ago
7

A 40.5 g sample of aluminum is cooled 7.5°C. The specific heat capacity of aluminum is

Chemistry
1 answer:
sweet-ann [11.9K]3 years ago
3 0
Q=mc\Delta T
Q= 40.5g x 0.900 J/g degree Celsius x 7.5
Q= 273.4 J.
Even if it is cooled , we use the same temperature as heating it.
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A breakfast of cereal, orange juice, and milk might contain 230 nutritional Calories. How much is this in Joules?
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Answer:

B

Explanation:

962,320 J

230 nutritional Calories in Joules is 962,320 J

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The kinetic molecular theory states that all particles of an ideal gas are
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THE KINETIC MOLECULAR THEORY STATES THAT ALL PARTICLES OF AN IDEAL GAS ARE IN CONSTANT MOTION AND EXHIBITS PERFECT ELASTIC COLLISIONS.

Explanation:

An ideal gas is an imaginary gas whose behavior perfectly fits all the assumptions of the kinetic-molecular theory. In reality, gases are not ideal, but are very close to being so under most everyday conditions.

The kinetic-molecular theory as it applies to gases has five basic assumptions.

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5 0
3 years ago
2 The change in the velocity of an object is defined as its​
ollegr [7]

Answer:

Acceleration is the rate of change in velocity

3 0
3 years ago
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How do you make a model of something you cannot see?
Vedmedyk [2.9K]
You have to imagine it
8 0
2 years ago
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For the reaction
s2008m [1.1K]

Answer:

0.558mole of SO₃

Explanation:

Given parameters:

Molar mass of SO₃ = 80.0632g/mol

Mass of S = 17.9g

Molar mass of S = 32.065g/mol

Number of moles of O₂ = 0.157mole

Molar mass of O₂ = 31.9988g/mol

Unknown:

Maximum amount of SO₃

Solution

  We need to write the proper reaction equation.

           2S + 3O₂ → 2SO₃

We should bear in mind that the extent of this reaction relies on the reactant that is in short supply i.e limiting reagent. Here the limiting reagent is the Sulfur, S. The oxygen gas would be in excess since it is readily availbale.

So we simply compare the molar relationship between sulfur and product formed to solve the problem:

First, find the number of moles of Sulfur, S:

   Number of moles of S = \frac{mass }{molar mass}

   Number of moles of S =  \frac{17.9 }{32.065} = 0.558mole

Now to find the maximum amount of SO₃ formed, compare the moles of reactant to the product:

       2 mole of Sulfur produced 2 mole of SO₃

   Therefore; 0.558mole of sulfur will produce 0.558mole of SO₃

5 0
3 years ago
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