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3 years ago

11

What the different betwen observe and reference

1 answer:

NNADVOKAT [17]3 years ago

7 0

Observe to to gather facts, by paying close attention towards what you are working on.

meanwhile, reference is the act or process on reaching to your conclusion, based on facts you already know .

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2 H2(g) + O2(g) 2 H2000

guajiro [1.7K]

A. 2 x 3 = 6 mol H2O

4 0

2 years ago

Which model failed to explain the

11Alexandr11 [23.1K]

Answer:

C). The Bohr-Rutherford model

Explanation:

The 'Bohr-Rutherford model' of the atom failed to elaborate on the attraction between some substances. It essentially targeted hydrogen atoms and failed to explain its stability across multi-electrons. The nature and processes of the chemical reactions remained unillustrated and thus, this is the key drawback of this model. Thus, <u>option C</u> is the correct answer.

5 0

3 years ago

Someone please answer i’ll give brainliest

Viktor [21]

Answer:

A) wrong. The molar is same so A is hevier

B)

Explanation:

Xg/mol × (same molar)= g

→ bigger molar bigger mass

8 0

2 years ago

A 57.9 g sample of glass is cooled by 27.0°C. How much heat does it release?

liberstina [14]

Explanation:

A 57.9 g sample of glass is cooled by 2.70'C how much heat does it release

1560

3 0

3 years ago

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2(l) → 2H2O(l) + O2(g) ΔH =

Mashcka [7]

<u>Answer:</u> The amount of heat released is -7.203 kJ

<u>Explanation:</u>

The given chemical equation follows:

$2H_2O_2(l)\rightarrow 2H_2O(l )+O_2(g);\Delta H=-196kJ$

To calculate the enthalpy change for 1 mole of the hydrogen peroxide, we use unitary method:

When 2 moles of hydrogen peroxide is reacted, the enthalpy of the reaction is -196 kJ

So, when 1 mole of hydrogen peroxide will react, the enthalpy of the reaction will be $\frac{-196}{2}\times 1=-98kJ$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of hydrogen peroxide = 2.50 g

Molar mass of hydrogen peroxide = 34 g/mol

Putting values in above equation, we get:

$\text{Moles of hydrogen peroxide}=\frac{2.50g}{34g/mol}=0.0735mol$

To calculate the heat of the reaction, we use the equation:

$\Delta H_{rxn}=\frac{q}{n}$

where,

$q$ = amount of heat released

n = number of moles = 0.0735 moles

$\Delta H_{rxn}$ = enthalpy change of the reaction = -98 kJ/mol

Putting values in above equation, we get:

$-98kJ/mol=\frac{q}{0.0735mol}\\\\q=(-98kJ/mol\times 0.0735mol)=-7.203kJ$

Hence, the amount of heat released is -7.203 kJ

8 0

3 years ago