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3 years ago

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Example 4. Balance the equation below in which methane reacts with oxygen in the atmosphere to release heat and the atoms recomb

ine to form carbon dioxide and water vapour. CH4 + O2------>CO2 + H2O 1 10

2 answers:

bija089 [108]3 years ago

5 0

Answer:

CH4+O2---->CO2 + H2O unbalance

C=1. C=1

H=4. H=2x2

O=2x2. O=2 +(1 x2)

CH4+2O2----->CO2 +2H2O. Balanced

Tems11 [23]3 years ago

4 0

Answer:

CH4 + 2O2 ----> CO2 + 2H2O

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Which trend is observed as the first four elements in Group 17 on the Periodic Table are considered in order of increasing atomi

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3 years ago

7. Which of the following represents the largest mass?

Tamiku [17]

Answer:

10kg = 10 x 1000 = 10,000g

Explanation:

To know the quantity with the largest mass, we have to express all the units in grams:

for: 2 x 10mg = 2 x 10 x 10⁻³ = 0.02g

0.001kg = 0.001 x 1000 = 1g

1 x 10⁵ng = 1 x 10⁵ x 10⁻⁹ = 0.0001g

2 x 10²cg = 2 x 10² x 10⁻² = 2g

10kg = 10 x 1000 = 10,000g

Note:

10⁻ ¹ deci(d)

10⁻² centi(c)

10⁻³ milli(m)

10⁻⁹ nano(n)

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5 0

4 years ago

The molecular weight of a gas that has a density of 5.75 g/l at stp is __________ g/mol.

Ira Lisetskai [31]

Answer : The molecular weight of a gas is, 128.9 g/mole

Explanation : Given,

Density of a gas = 5.75 g/L

First we have to calculate the moles of gas.

At STP,

As, 22.4 liter volume of gas present in 1 mole of gas

So, 1 liter volume of gas present in $\frac{1}{22.4}=0.0446$ mole of gas

Now we have to calculate the molecular weight of a gas.

Formula used :

$\text{Moles of gas}=\frac{\text{Mass of a gas}}{\text{Molecular weight of a gas}}$

Now put all the given values in this formula, we get the molecular weight of a gas.

$0.0446mole=\frac{5.75g}{\text{Molecular weight of a gas}}$

$\text{Molecular weight of a gas}=128.9g/mole$

Therefore, the molecular weight of a gas is, 128.9 g/mole

8 0

3 years ago

Read 2 more answers

3. Given 20g of Barium Hydroxide, how many grams of

anastassius [24]

The number of grams of ammonium nitrate (NH₄NO₃) it would take for all the barium hydroxide to react is 18.7g

First, we will write the balanced chemical equation for the reaction

The balanced chemical equation for the reaction is

Ba(OH)₂ + 2NH₄NO₃ → 2NH₄OH + Ba(NO₃)₂

This means, 1 mole of barium hydroxide is required to react with 2 moles of ammonium nitrate

Now, we will calculate the number of moles of barium hydroxide present.

Mass of barium hydroxide (Ba(OH)₂) = 20 g

Using the formula

$Number\ of\ moles = \frac{Mass}{Molar\ mass}$

Molar mass of Ba(OH)₂ = 171.34 g/mol

∴ Number of moles of Ba(OH)₂ present = $\frac{20}{171.34}$

Number of moles of Ba(OH)₂ present = 0.116727 mole

Now,

Since 1 mole of barium hydroxide is required to react with 2 moles of ammonium nitrate

Then,

0.116727 mole of barium hydroxide will react with 2 × 0.116727 mole of ammonium nitrate

2 × 0.116727 = 0.233454 mole

∴ Number of moles of NH₄NO₃ required is 0.233454 mole

Now, for the mass of ammonium nitrate (NH₄NO₃) required

From the formula

Mass = Number of moles × Molar mass

Molar mass of NH₄NO₃ = 80.043 g/mol

∴ Mass of NH₄NO₃ required = 0.233454 × 80.043

Mass of NH₄NO₃ required = 18.68636 g

Mass of NH₄NO₃ required ≅ 18.7g

Hence, the number of grams of ammonium nitrate (NH₄NO₃) it would take for all the barium hydroxide to react is 18.7g

Learn more on determining mass of reactant required here: brainly.com/question/11232389

6 0

2 years ago