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3 years ago

Is a squirrel eating acorns and a fire burning a good examples of chemical energy

Chemistry

2 answers:

Snowcat [4.5K]3 years ago

6 0

Answer:

yes

Explanation:

Fire that burns is a very good example

pentagon [3]3 years ago

5 0

Answer:

Definitely the fire burning is.

Explanation:

It’s a chemical combustion

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What is Gram Atomic mass ?

KIM [24]

Answer:

Gram atomic mass of an element can be defined as the mass of one mole of atoms of a particular element. It is numerically equivalent to the value of the element's atomic mass unit but has its unit in grams.

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2 years ago

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Consider a hypothetical reaction in which A and B are reactants, and C and D are products. If 26 grams of A completely reacts wi

natali 33 [55]

Answer:

The answer to your question is: 24 grams of D

Explanation:

To answer this question we need to remember the Lavoisier law of conservation of mass, which says that in a chemical reaction matter is neither created nor destroyed.

This means that the amount of matter stays the same.

Then, the reaction is

A + B ⇒ C + D

26 g 12 g 14 g x

mass

of reactants 38 g ? mass of products, but it must be

equal to the mass of products

Then 14g + x = 38

x = 38 - 14

x = 24 g of D

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3 years ago

What is a fusion reaction

Liula [17]

When two atoms of Hydrogen combine together, or fuse, they make an atom of Helium.

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3 years ago

Vocabulary

mihalych1998 [28]

Answer:

the only one i really know is magna carta which is an article created so that the king's power could be limited or something

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3 years ago

At 25°C, K = 0.090 for the following reaction. H2O(g) + Cl2O(g) equilibrium reaction arrow 2 HOCl(g) Calculate the concentration

wlad13 [49]

Answer:

[HOCl] = 0.00909 mol/liter

[H₂O] = 0.03901 mol/liter

[Cl₂O] = 0.02351 mol/liter

Explanation:

1. Chemical reaction:

$H_2O(g)+Cl_2O(g)\rightleftharpoons 2 HOCl(g)$

2. Initial concentrations:

i) 1.3 g H₂O

Number of moles = 1.3g / (18.015g/mol) = 0.07216 mol

Molarity, M = 0.07216 mol / 1.5 liter = 0.0481 mol/liter

ii) 2.2 g Cl₂O

Number of moles = 2.2 g/ (67.45 g/mol) = 0.0326 mol

Molarity = 0.0326mol / 1.5 liter = 0.0217 mol/liter

3. ICE (Initial, Change, Equilibrium) table

$H_2O(g)+Cl_2O(g)\rightleftharpoons 2 HOCl(g)$

I 0.0481 0.0326 0

C -x -x +x

E 0.0481-x 0.0326-x x

4. Equilibrium expression

$K_c=\dfrac{[HOCl]^2}{[H_2O].[Cl_2O]}$

$0.09=\dfrac{x^2}{(0.0481-x)(0.0326-x)}$

5. Solve:

$x^2=0.09(x-0.0481)(x-0.0326)\\\\0.91x^2+0.007263x-0.000141125=0$

Use the quadatic formula:

$x=\dfrac{-0.007263\pm \sqrt{(0.007263)^2-4(0.91)(-0.000141125)}}{2(0.91)}$

The positive result is x = 0.00909

Thus the concentrations are:

[HOCl] = 0.00909 mol/liter

[H₂O] = 0.0481 - 0.00909 = 0.03901 mol/liter

[Cl₂O] = 0.0326 - 0.00909 = 0.02351 mol/liter

3 0

3 years ago