1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
8090 [49]
3 years ago
14

Consider the combustion of octane (C8H18)

Chemistry
1 answer:
Masja [62]3 years ago
8 0
First, you have to find now many moles of octane are present in 191.6g of octane.  To do this you need to do this you need to divide 191.6g by its molar mass (which is 114g/mol).  This will give you 1.681 moles of octane.  Then you need to use the fact that 2 moles of octane are us ed to make 16 moles of carbon dioxide to find how many moles of carbon dioxide 1.681mole of octane produces. To do this you need to multiply 1.681mole by 16/2 to get 13.45mol carbon dioxide.  The final step is to find the number of grams presswnt in 13.446 moles of carbon dioxide.  To do this you need to multiply 13.446 mole by carbon dioxides molar mass (which is 44g/mol) to get 591.6 g of carbon dioxide.
Therefore, 591.6g of carbon dioxide is produced when 191.6 grams of octane is burned.

I hope this helps. Let me know in the comments if anything is unclear.
You might be interested in
Determine how many grams of N2 are produced from the reaction of 8.37 g of H2O2 and 5.29 g of N2H4.
Dmitriy789 [7]
N₂H₄  +  2H₂O₂    →   N₂  +  4H₂O

mol = mass ÷ molar mass

If mass of hydrazine (N₂H₄)  = 5.29 g 
then mol of hydrazine           = 5.29 g ÷ ((14 ×2) + (1 × 4))
                                              = 0.165 mol

mole ratio of hydrazine to Nitogen is     1   :  1
  ∴ if moles of hydrazine = 0.165 mol
     then moles of nitrogen = 0.165 mol

Mass = mol × molar mass

Since mol of nitrogen (N₂)  = 0.165
then mass of hydrazine      = 0.165 × (14 × 2)
                                           = 4.62 g
5 0
2 years ago
Given 16.2 grams of substance Y, if the substance absorbs 2722 joules of energy and the specific heat of the substance is 9.22 J
snow_tiger [21]
Since the substance absorbs heat, it is expected that the temperature will rise. The formula for the internal energy of a substance is given by the equation:

ΔU = mCpΔT

where:

ΔU = internal energy
m = mass of substance
Cp = specific heat capacity of substance
ΔT = change in temperature

ΔU = 2722 Joules = 16.2 grams (9.22 J/g-°C) (Tf - 26°C)

This gives a final temperature of Tf = 44.22 °C
4 0
3 years ago
3 A soil has 70% sand, 20% silt
Kisachek [45]

Today, as part of the series of posts on soils, we are going to look at ‘soil texture’. Soil forms the basis for all life but it’s important to know about its mineral constitution as well as its biological profile.

Texture refers to the ‘feel’ of the soil. This is affected by the constituent materials found within it, specifically sand, silt and clay particles. A coarse sand will feel gritty but a wet clay will feel heavy and sticky. The texture of a soil has a direct impact on the way the soil reacts to certain environmental conditions – for example, towards drought or heavy rain (with sandy soils more freely draining).

There is a big difference in the size of the different particles.

Coarse sand = diameter 2-0.2mm

Fine sand = diameter 0.2-0.02mm

Silt = diameter 0.02-0.002mm

Clay = diameter less than 0.002mm

Note how the clay particles are much smaller than the sand particles – this is important as it means the total surface area of a clay soil is much greater and so the capacity to hold water is also much greater.

Between the sand, silt and clay particles there are lots of pores. In fact a soil as a whole is generally 45% mineral, 5% organic matter (depending on the soil) and 50% pore space through which air and water can pass.

Sand –

Made up of weathered primary rock minerals.

The particles are irregular in outline.

They are large and so do not pack together easily.

Large pore spaces in between.

Air gets in very easily and water flows rapidly through it.

Silt –

7 0
3 years ago
What is the ideal gas law
dlinn [17]

Answer: Gases are complicated. They're full of billions and billions of energetic gas molecules that can collide and possibly interact with each other. Since it's hard to exactly describe a real gas, people created the concept of an Ideal gas as an approximation that helps us model and predict the behavior of real gases. The term ideal gas refers to a hypothetical gas composed of molecules which follow a few rules:

Ideal gas molecules do not attract or repel each other. The only interaction between ideal gas molecules would be an elastic collision upon impact with each other or an elastic collision with the walls of the container. [What is an elastic collision?]

Ideal gas molecules themselves take up no volume. The gas takes up volume since the molecules expand into a large region of space, but the Ideal gas molecules are approximated as point particles that have no volume in and of themselves.

If this sounds too ideal to be true, you're right. There are no gases that are exactly ideal, but there are plenty of gases that are close enough that the concept of an ideal gas is an extremely useful approximation for many situations. In fact, for temperatures near room temperature and pressures near atmospheric pressure, many of the gases we care about are very nearly ideal.

If the pressure of the gas is too large (e.g. hundreds of times larger than atmospheric pressure), or the temperature is too low (e.g.

−

200

C

−200 Cminus, 200, start text, space, C, end text) there can be significant deviations from the ideal gas law.

Explanation:

7 0
2 years ago
Read 2 more answers
A sugar cube was placed into a beaker containing 100 mL of water at room temperature and completely dissolved into the water. Th
Bad White [126]

Answer:

Boil the water until it evaporates

Explanation:

If the water evaporates the sugar will no longer bond to it and then percipitate at the bottom of the beaker.

3 0
3 years ago
Other questions:
  • What are the reagents for BaCO3(s)
    7·1 answer
  • An aqueous solution has a mass of 490 grams containing 8.5 × 10-3 gram of calcium ions. The concentration of calcium ions in thi
    9·1 answer
  • What caused the bonding of two atoms which undergo an ionic bond?
    10·1 answer
  • Consider the reaction 2 CO + O2 → 2 CO2 .What is the percent yield of carbon dioxide
    10·1 answer
  • What is considered to be an unsafe level of lead in flint michigan water?
    14·1 answer
  • Help please! I don’t understand this
    11·1 answer
  • Ideal gas (n 2.388 moles) is heated at constant volume from T1 299.5 K to final temperature T2 369.5 K. Calculate the work and h
    13·1 answer
  • Balance the following chemical reaction: _NaOH + _H2SO4 ----->_Na2SO4 +_H20
    6·1 answer
  • Suggest an alternative to zinc oxide that could react with hydrochloric acid to give you the desirable product.
    12·1 answer
  • Can the element gold kick out magnesium from a compound?
    6·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!