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velikii [3]
3 years ago
11

In a combustion analysis, the carbon in a hydrocarbon fuel is

Chemistry
1 answer:
scoray [572]3 years ago
7 0
During a combustion reaction the carbon in a hydrocarbon compound is paired with Oxygen (O2) in the air to form Carbon-Dioxide (CO2), whilst the Hydrogen too pairs with Oxygen to form water vapour (H2O). Heat is also produced during this reaction.
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atroni [7]

Answer:

A?

Explanation:

7 0
2 years ago
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10 examples of<br>combination reaction​
Alla [95]

You can easily find hundreds on the internet.

4 0
3 years ago
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A 3.0 g sample of a gas occupies a volume of 1.00L at 100C and 740 torr pressure. The molecular weight of the
SOVA2 [1]

Answer:

94.2 g/mol

Explanation:

Ideal Gases Law can useful to solve this

P . V = n . R . T

We need to make some conversions

740 Torr . 1 atm/ 760 Torr = 0.974 atm

100°C + 273 = 373K

Let's replace the values

0.974 atm . 1 L = n . 0.082 L.atm/ mol.K . 373K

n will determine the number of moles

(0.974 atm . 1 L) / (0.082 L.atm/ mol.K . 373K)

n = 0.032 moles

This amount is the weigh for 3 g of gas. How many grams does 1 mol weighs?

Molecular weight → g/mol → 3 g/0.032 moles = 94.2 g/mol

3 0
3 years ago
For an ideal gas condition, what is the mass (g) of N2 if the pressure is 2.0 atm, the volume is 25 mL and the temperature is 29
Alchen [17]

Answer:

THE MASS OF NITROGEN GAS IN THIS CONDITIONS IS 0.0589 g

Explanation:

In an ideal condition

PV = nRT or PV = MRT/ MM where:

M = mass = unknown

MM =molar mass = 28 g/mol

P = pressure = 2 atm

V = volume = 25 mL = 0.025 L

R = gas constant = 0.082 L atm/mol K

T = temperature = 290 K

n = number of moles

The gas in the question is nitrogen gas

Molar mass of nitrogen gas = 14 * 2 = 28 g/mol

Then equating the variables and solving for M, we have

M = PV MM/ RT

M = 2 * 0.025 * 28 / 0.082 * 290

M = 1.4 / 23.78

M = 0.0589 g

The mass of the nitrogen gas at ideal conditions of 2 atm, 25 mL volume and 290 K temperature is 0.0589 g

3 0
3 years ago
Please help me don’t scam
rosijanka [135]

Answer:b

Explanation:

4 0
3 years ago
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