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2 years ago

What happens when something warm up

Chemistry

1 answer:

Anna [14]2 years ago

4 0

Answer:

Heat, once absorbed as energy, contributes to the overall internal energy of the object. One form of this internal energy is kinetic energy; the particles begin to move faster, resulting in a greater kinetic energy. This more vigorous motion of particles is reflected by a temperature increase.

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Mrs. Rushing has 3 chemistry classes with 24 students in each. An experiment calls for each student to use 4 test tubes. How man

stira [4]

If they have 3 chemistry classes with 24 students, than there are 72 students in total. Each student requires 4 test tubes. 72 * 4 = 288 test tubes. Our answer is C.) 288 test tubes

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4 years ago

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A 1.2516 gram sample of a mixture of caco3 and na2so4 was analyzed by dissolving the sample and completely precipitating the ca

Dennis_Churaev [7]

Answer:

0.009725 moles of H2C2O4

0.009725 moles CaCO3

Mass percentage = 77.77%

Explanation:

Step 1: The balanced equation

2MnO4- +5C2H2O4+6H+ →2Mn2+ +10CO2+8H2O

We can see that for 2 moles of Mno4- consumed , there is 5 moles of C2H2O4 needed and 6 moles H+ to produce 2 moles Mn2+, 10 moles of CO2 and 8 moles of H2O

Step 2: Calculate moles of MnO4-

Molarity = Moles/volume

Moles of Mno4- = Molarity of MnO4- * Volume of Mno4-

Moles of Mno4- = 0.1092M * 35.62 *10^-3 L

Moles of MnO4- = 0.00389 moles

Step 3: Calculate moles of H2C2O4

Since there is needed 5 moles of C2H2O4 to consume 2 moles of MnO4-

then for 0.00389 moles of MnO4-, there is 5/2 *0.00389 = 0.009725 moles of H2C2O4

Step 4: Calculate moles of CaCO3

moles of H2C2O4 = moles CaCO3, therefore, 0.009725 moles H2C2O4 = 0.009725 moles CaCO3

Step 5: Calculate mass of CaCO3

Molar mass of CaCO3 = 100.09 g/mole

Mass of CaCO3 = moles of CaCO3 * Molar mass of CaCO3

Mass of CaCO3 = 0.009725 moles * 100.09 g/mole = 0.9734 g

Step 6: Calculate percentage by weight of CaCO3

Mass of CaCO3 = 0.9734g

Mass of original sample = 1.2516g

Mass percentage = 0.9734/1.2516 *100% = 77.77%

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4 years ago

If the heat of fusion for water is 334 j/g, how many Jules are needed to melt 45.0 g of ice at 0.0°c?

finlep [7]

Given parameters:

Heat of fusion of water = 334j/g

Mass of ice = 45g

Temperature of ice = 0.0°c

Unknown:

Amount of heat needed to melt = ?

Solution:

This is simply a phase change and a latent heat is required in this process.

To solve this problem; use the mathematical expression below;

H = mL

where m is the mass

L is the heat of fusion of water;

H = 45 x 334 = 15030J

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3 years ago

8. Which of the following is TRUE about limiting and excess reactants?

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B. The limiting reactant determines the max amount of product that can be formed

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This will be classified as light on the API scale due to the large percentage of lighter fractions such as paraffins and naphthenes.

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4 years ago

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What happens when something warm up​

What happens when something warm up