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3 years ago

Please give me your best chemistry joke. The best joke gets Brainlest.

Chemistry

2 answers:

stepan [7]3 years ago

7 0

Answer:

why cant you trust molecules?

Explanation:

they are big liars.

tia_tia [17]3 years ago

5 0

Answer:

why can you never trust a atom

Explanation:

they make everything up

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How many molecules are in 0.79 moles of NH4?

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Answer:

Explanation:

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3 years ago

How to solve for enthalpy for changes

Natasha_Volkova [10]

Always use this method !!! always

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4 years ago

What happens when hydrogen reacts with nitrogen at necessary conditions.

Orlov [11]

Answer:

When hydrogen gas combines with nitrogen to form Ammonia the following chemical reaction will take place. Our equilibrium reaction will be N2(g) + 3H2(g) ⇔ 2NH3(g) + Heat. In this case, Hydrogen and nitrogen react together to form ammonia.

Explanation:

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3 years ago

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Oxalic Acid, a compound found in plants and vegetables such as rhubarb, has a mass percent composition of 26.7% C, 2.24% H, and

blondinia [14]

Answer:

HCO₂

Explanation:

From the information given:

The mass of the elements are:

Carbon C = 26.7 g; Hydrogen H = 2.24 g Oxygen O = 71.1 g

To determine the empirical formula;

First thing is to find the numbers of moles of each atom.

For Carbon:

$=26.7 \ g\times \dfrac{1 \ mol }{12.01 \ g} \\ \\ =2.22 \ mol \ of \ Carbon$

For Hydrogen:

$=2.24 \ g\times \dfrac{1 \ mol }{1.008 \ g} \\ \\ =2.22 \ mol \ of \ Hydrogen$

For Oxygen:

$=71.1 \ g\times \dfrac{1 \ mol }{1.008 \ g} \\ \\ =4.44 \ mol \ of \ oxygen$

Now; we use the smallest no of moles to divide the respective moles from above.

For carbon:

$\dfrac{2.22 \ mol \ of \ carbon}{2.22} =1 \ mol \ of \ carbon$

For Hydrogen:

$\dfrac{2.22 \ mol \ of \ carbon}{2.22} =1 \ mol \ of \ hydrogen$

For Oxygen:

$\dfrac{4.44 \ mol \ of \ Oxygen}{2.22} =2 \ mol \ of \ oxygen$

Thus, the empirical formula is HCO₂

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3 years ago

What is the percent by mass of oxygen in carbon dioxide (CO2)?

krok68 [10]

Answer:

I think that it will be

Explanation:

72.71%

8 0

3 years ago

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