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3 years ago

Provide an example of a substance with non-polar bonds

Chemistry

1 answer:

LenaWriter [7]3 years ago

5 0

Answer:

Tin (IV) chloride (SnCl4)...Methane(CH4)

Explanation:

all the dipole moments of the bonds tend to cancel each other out...hence leaving the substance non-polar

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Can someone please help me with this asap, it’s due today please help me

hammer [34]

Answer:

lol I hate chemical but let me give some advice

Explanation:

Please go on Khan Academy or look at your notes and I promise you can figure out! Seriously, I am trying to be helpful not like the annoying teacher that says "figure it out"

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3 years ago

Why are supergiant so bright?

Yuliya22 [10]

Because supergiants are so massive, the core temperature gets much hotter than in giants, so supergiants can fuse elements heavier than hydrogen and helium. But to support their tremendous mass, supergiants burn up their fuel much more quickly.

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3 years ago

Read 2 more answers

5. In an oxyacetylene welding torch, acetylene (C2H2) burns in pure oxygen with a very hot flame. The reaction is: 2 C2H2 + 5 O2

gulaghasi [49]

11.375 g ethylene is consumed if 35.0 grams of oxygen is allowed to react and 7.875 ml of water will be produced when the 35.0 grams of oxygen is allowed to react.

<h3>What are moles?</h3>

A mole is defined as 6.02214076 × $10^{23}$ of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.

According to the chemical equation for the combustion of ethylene, 5

moles of oxygen are required to react with 2 moles of ethylene, hence

$m_{_C_2_H_2}$ $= 35gX \frac{1 mol}{(2 \;X\; 16)g } X \frac{2 mol}{(5\;mol )} X \frac{26g}{1 mol }$

$m_{_C_2_H_2} = 11.375 g$

Similarly, 5 moles of oxygen are required as a reactant to produce 2 moles of water, thus

$m_{_H_2_O} = 35gX \frac{1 mol}{(2 \;X\; 16)g } X \frac{2 mol}{(5\;mol )} X \frac{18g}{1 mol }$

$m_{_H_2_O} = 7.875 g$

Given that the density of water is $1.0g ml^{-1}$ , therefore

$Density = \frac{Mass \;of \;water}{Volume \;of \;water}$

$Volume \;of \;water = \frac{7.875}{1.0 g ml^{-1}}$

The volume of water = 7.875 ml

Learn more about moles here:

brainly.com/question/8455949

#SPJ1

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2 years ago

Read 2 more answers

A student tested a 0.1 M aqueous solution and made the following observations:

liberstina [14]

A student tested a 0.1 M aqueous solution and made the following observations conducts electricity, turns blue litmus to red and reacts with Zn(s) to produce gas bubbles. The compound that could be the solute in this solution is HBr. The answer is number 3.

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3 years ago

Using a chemical equation to find moles of product from moles...

kaheart [24]

Answer: 0.600 moles

Balanced eqn for decomposition of the rocket fuel:

2 NH4ClO4 (s) ----> N2 (g) + Cl2 (g) + 2 O2 (g) + 4 H2O (g)

Since, 2 moles of NH4ClO4 produces 2 moles of O2 gas, this means that 0.6 moles of NH4ClO4 will produce 0.6 moles of O2 gas

7 0

2 years ago