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3 years ago

From his experiments j.j. Thomson conclude that

Chemistry

2 answers:

nevsk [136]3 years ago

8 0

Answer:

J.J. Thomson could conclude that most of the mass of an atom is concentrated in its center, or the area where most of the parts of an atom such as the nucleus

Explanation:

musickatia [10]3 years ago

3 0

Answer:

J.J. Thomson's experiments with cathode ray tubes showed that all atoms contain tiny negatively charged subatomic particles or electrons. Thomson proposed the plum pudding model of the atom, which had negatively-charged electrons embedded within a positively-charged "soup."

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Give two reasons why quarrying is bad for the environment?

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1) The longer the quarrying goes on the less and less recources we will have, soon leading to no more recources

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2 years ago

2.0g divided by 34.0 g times 100% equals what?

Lubov Fominskaja [6]

Answer: $\frac{1}{17}$

Explanation: \frac{2}{34}\cdot \:100\%\:=\frac{1}{17}

I tried my best, I hope this helps!

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3 years ago

Form the complementary solution to the homogeneous equation. yc(t) = Cl [ ] +C2 Construct the (simplest) particular olution of t

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Answer:

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Explanation:

Please kindly check attachment for the step by step solution of the given problem.

6 0

3 years ago

What is the volume of SO3 in 835 g SO3?

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2 years ago

Stearic acid (C18H36O2) is a fatty acid, a molecule with a long hydrocarbon chain and an organic acid group (COOH) at the end. I

Paha777 [63]

Answer:

There is 9671 Kj of heat released

Explanation:

Step 1: The balanced equation:

C18H36O2(s) + 26O2(g) --> 18CO2(g)+18H2O(g)

This means for 1 mole of C18H36O2 consumed there is 26 moles of O2 needed to produce 18 moles of CO2 and 18 moles of H2O.

Step 2: Calculate the heat of combustion

ΔH (combustion) = [18*(ΔHf of CO2) + 18*(ΔHf of H2O)] - [1*(ΔHf of C18H36O2) + 26*(ΔHf of O2)]

ΔH (combustion) = [18*(-394 kJ/mol) + 18*(-242 kJ/mol)] - [1*(-948 kJ/mol) + 26*(0 kJ/mol)]

ΔH (combustion) = [(-7092 kJ/mol) + (-4356 kJ/mol)] - (-948 kJ/mol)

= -10500 kJ/mol

ΔH (combustion) = heat released / number of moles of stearic acid

Step 3: Calculate moles of stearic acid

moles of stearic acid = mass / Molar mass of stearic acid

moles of stearic acid = 262g / 284.48 g/mole = 0.921 moles

Step 4: Calculate moles of oxygen

moles of O2 = 914.5 / 32g/mole

moles of O2 = 28.578125 moles

Stearic acid is the limiting reactant: it will completely react

There will react 26*0.921 mole = 23.946 mole of O2

This means there will remain 4.63 moles of O2

Step 5: Calculate heat released

q = (ΔH combustion) * (moles of stearic acid) = (-10500 kJ/mol) * (0.921 moles) = 9671 Kj

There is 9671 Kj of heat released

6 0

2 years ago