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3 years ago

How do i calculate the mass of CO2 emitted per Kj of heat produced in a combustion reaction?

1 answer:

6 0

methanol:

1 mole CH3 OH --> produces --> 1 mole CO2

1 mole CO2 has a molar mass of 44.01 gh/mole

your set up is:
(44.01 g CO2) / -726.5kJ = 0.06058g

your answer 0.06058 grams of CO2 produced per kJ released.

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2 Carbon (C) is found on the Periodic Table; however, Carbon Dioxide (CO2) is not. Why is this the case? А B с D

ad-work [718]

Answer:

2 Carbon (C) is found on the Periodic Table; however, Carbon Dioxide (CO2) is not. Why is this the case? А B с D

A Only substances that cannot be broken down into simpler substances are found on the Periodic Table.

B Only gases are found on the Periodic Table.

C Only compounds are found on the Periodic Table.

D Compounds cannot be broken down into simpler substances.

Answer:

Explanation:

8 0

2 years ago

The following reaction shows calcium chloride reacting with silver nitrate.

adell [148]

Grams of Ca(NO₃)₂ produced : 0.985 g

<h3>Further explanation</h3>

A reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.

Reaction

CaCl₂ + 2AgNO₃ → 2AgCl + Ca(NO₃)₂

MW AgNO₃ : 107.9+14+3.16=169.9

mol AgNO₃ :

$\tt \dfrac{2}{169.9}=0.012$

mol ratio Ca(NO₃)₂ : AgNO₃ = 1 : 2, so mol Ca(NO₃)₂ :

$\tt \dfrac{1}{2}\times 0.012=0.006$

MW Ca(NO₃)₂ : 40.1+2.14+6.16=164.1 g/mol

mass Ca(NO₃)₂ :

$\tt 0.006\times 164.1=0.985$

7 0

3 years ago

Heeellllpppp ASAP ......

iren [92.7K]

Answer:

I saw B, he vented SUS

Explanation:

Iodoethane Is the answer.

7 0

3 years ago

To reduce competition, an organism can do which of the following?

andrew-mc [135]

Answer:

sorry cant help

Explanation:

4 0

3 years ago

Dihydrogen dioxide decomposes into water and oxygen gas. Calculate the amounts requested if 1.34 moles of dihydrogen dioxide rea

a_sh-v [17]

Answers:

a. Moles of oxygen formed: 0.670 mol

b. Moles of water formed: 1.34 mol

c. Mass of water formed: 24.1 g

d. Mass of oxygen formed: 21.4 g

Explanation:

Dihdyrogen dioxide is the chemical name for a compound made of two hydrogen atoms and two oxide atoms, i.e. H₂O₂, which is also known as hydrogen peroxide or oxygenated water.

The decomposition reaction of dihydrogen dioxide into water and oxygen gas is represented by the balanced chemical equation:

$2H_2O_2(l)\rightarrow 2H_2O(l)+O_2(g)$

The mole ratios derived from that balanced chemical equation are:

2 mol H₂O₂ : 2 mol H₂O : 1 mol O₂

a. Moles of oxygen formed

Set the proportion using the theoretical mole ratio of H₂O₂ to O₂ and the amount of moles of dyhydrogen dioxide that react:

$2\text{ mol }H_2O_2/1\text{ mol }O_2=1.34\text{ mol }H_2O_2/x$

When you solve for x, you get:

x = 1.34 mol H₂O₂ × 1 mol O₂ / 2 mol H₂O₂ = 0.670 mol O₂

b. Moles of water formed

Set the proportion using the theoretical mole ratio of H₂O₂ to H₂O and the amount of moles of dyhydrogen dioxide that react:

$2\text{ mol }H_2O_2/2\text{ mol }H_2O=1.34\text{ mol }H_2O_2/x$

When you solve for x, you get:

x = 1.34 mol H₂O₂ × 2 mol H₂O / 2 mol H₂O₂ = 1.34 mol H₂O

c. Mass of water formed

Using the number of moles of water calculated in the part b., you calculate the mass of water formed, in grams, using the molar mass of water:

Molar mass of water = 18.015 g/mol

Number of moles = mass in grams / molar mass

⇒ mass in grams = number of moles × molar mass

⇒ mass in grams = 1.34 mol × 18.015 g/mol = 24.1 g

d. Mass of oxygen formed

Using the number of moles of oxygen determined in the part a., you calculate the mass in grams using the molar mass of O₂.

Molar mass of O₂ = 32.00 g/mol

mass = molar mass × number of moles

mass = 32.00 g/mol × 0.670 mol = 21.4 g.

5 0

3 years ago