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3 years ago

I REALLY NEED HELP WITH THIS CHEMESTRY PROJECT. I DO NOT UNDERSTAND ANYTHING OF THIS. CAN YOU GUYS PLZ HELP ME?

Chemistry

2 answers:

ivanzaharov [21]3 years ago

8 0

I AGREE WITH bmstanley19

den301095 [7]3 years ago

7 0

You should up the points because its challenging
ill try to help

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Gaseous ethane (CH,CH,) will react with gaseous oxygen (0,) to produce gaseous carbon dioxide (CO) and gaseous water (H2O). Supp

notka56 [123]

Answer:

0.00 g

Explanation:

We have the masses of two reactants, so this is a limiting reactant problem.

We will need a balanced equation with masses, moles, and molar masses of the compounds involved.

1. Gather all the information in one place with molar masses above the formulas and masses below them.

Mᵣ 30.07 32.00

2CH₃CH₃ + 7O₂ ⟶ 4CO₂ + 6H₂O

Mass/g: 1.50 11.

2. Calculate the moles of each reactant

$\text{moles of C$_{2}$H}_{6} = \text{1.50 g C$_{2}$H}_{6} \times \dfrac{\text{1 mol C$_{2}$H}_{6}}{\text{30.07 g C$_{2}$H}_{6}} = \text{0.04988 mol C$_{2}$H}_{6}\\\\\text{moles of O}_{2} = \text{11. g O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{32.00 g O}_{2}} = \text{0.34 mol O}_{2}$

3. Calculate the moles of CO₂ we can obtain from each reactant

From ethane:

The molar ratio is 4 mol CO₂:2 mol C₂H₆

$\text{Moles of CO}_{2} = \text{0.04988 mol C$_{2}$H}_{6} \times \dfrac{\text{4 mol CO}_{2}}{\text{2 mol C$_{2}$H}_{6}} = \text{0.09976 mol CO}_{2}$

From oxygen:

The molar ratio is 4 mol CO₂:7 mol O₂

$\text{Moles of CO}_{2} = \text{0.34 mol O}_{2}\times \dfrac{\text{4 mol CO}_{2}}{\text{7 mol O}_{2}} = \text{0.20 mol CO}_{2}$

4. Identify the limiting and excess reactants

The limiting reactant is ethane, because it gives the smaller amount of CO₂.

The excess reactant is oxygen.

5. Mass of ethane left over.

Ethane is the limiting reactant. It will be completely used up.

The mass of ethane left over will be 0.00 g.

8 0

3 years ago

A 211 g sample of barium carbonate, baco3, reacts with a solution of nitric acid to give barium nitrate, carbon dioxide, and wat

bija089 [108]

Answer:
Mass = 47.04 g

Volume = 23.94 L

Solution:

The equation for given reaction is as follow,

BaCO₃ + 2 HNO₃ → Ba(NO₃)₂ + CO₂ + H₂O

According to this equation,

197.34 g (1 mole) BaCO₃ produces = 44 g (1 mole) of CO₂
So,
211 g of BaCO₃ will produce = X g of CO₂

Solving for X,
X = (211 g × 44 g) ÷ 197.34 g

X = 47.04 g of CO₂

As we know,

44 g (1 mole) CO₂ at STP occupies = 22.4 L volume
So,
47.04 g of CO₂ will occupy = X L of Volume

Solving for X,
X = (47.04 g × 22.4 L) ÷ 44 g

X = 23.94 L Volume

8 0

4 years ago

Pls help me here, thanks in advance

Marat540 [252]

Answer:

What's the problem???

4 0

3 years ago

Read 2 more answers

If you remove one bulb from a string of lights, all the remaining lights will go out. Are the lights in a series or parallel cir

Aleksandr [31]

Answer:

series bro. i think bro

6 0

3 years ago

Read 2 more answers

Guess how many water molecules self-ionize in one liter of water! a) 7 moles b) 1 mole c) 10,000,000 moles d) 0.0000001 moles

Rudiy27

Answer:

Explanation:

This seems like a weird question

Water is held together by covalent bonds. The amount of energy required to break these bonds so that water would split into it's respective ions is pretty high. The chances that any one of the molecules floating in 1L of water get enough energy to spontaneously burst into it's ions is slim to none.

So, D) seems like the most likely answer

6 0

3 years ago