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2 years ago

13

Please help me decode this. The question for this image is what is the code, and the code has to be: alphabetical without spaces

- all lower case

1 answer:

nata0808 [166]2 years ago

3 0

Answer:

c

Explanation:

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Explanation:

Catalyst is I2 . Because I2 is reacted with starting material in step 1 and generated in second step

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What is the total pressure in units of kPa in a 7.85 L container that contains 4.45 moles of N2 and 2.45 moles of O2 at a temper

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32.42

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2 years ago

How many molecules are in 1 mole of H2O

Olegator [25]

Answer:

A mole (mol) is the amount of a substance that contains 6.02 × 10 23 representative particles of that substance. The mole is the SI unit for the amount of a substance. There are, therefore, 6.02 × 10 23 water molecules in a mole of water molecules. Water (H2O) is made from 2 atoms of hydrogen and 1 atom of oxygen.

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2 years ago

Which of the following describe chemical properties? Check all that apply.

Mars2501 [29]

My answer will be B and D

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3 years ago

a quantity of zinc reacts with sulfuric acid and produces 0.10g of hydrogen. how many particles of zinc are required socratic.or

alekssr [168]

Answer:

grams of zinc required = 3.24 g

Particles of zinc required = $2.99\times 10^{22}$

Explanation:

Given that:-

Mass of hydrogen gas produced = 0.10 g

Calculation of the moles of $H_2$ as:-

Mass = 0.10 g

Molar mass of $H_2$ = 2.016 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{0.10\ g}{2.016\ g/mol}$

$Moles= 0.0496\ mol$

According to the reaction shown below:-

$Zn+H_2SO_4\rightarrow ZnSO_4+H_2$

1 mole of hydrogen gas is produced when 1 mole of zinc reacts

So,

0.0496 mole of hydrogen gas is produced when 0.0496 mole of zinc reacts

Moles of Zinc required = 0.0496 moles

Molar mass of zinc = 65.38 g/mol

mass= Moles*Molar mass = $0.0496\ moles\times 65.38\ g/mol=3.24\ g$

Also, 1 mole of Zinc contains $6.023\times 10^{23}$ particles

0.0496 mole of Zinc contains $0.0496\times 6.023\times 10^{23}$ particles

Particles of zinc required = $2.99\times 10^{22}$

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2 years ago