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3 years ago

Classify these bonds as ionic, polar covalent, or nonpolar covalent na-f

1 answer:

6 0

An ionic bond is a bond between two ions, one is positive charge and one is negative charge. A polar covalent bond is when 2 electrons are shared between 2 atoms but not in equal strength. A nonpolar covalent bond is when 2 atoms equally share 2 electrons.

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How far does light travel in 2.5 seconds

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299,792,458 meters per second

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How many grams is 10 moles of H2O?

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Answer:

So, 10 mole of water will weigh (18x10) = 180g.

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3 years ago

What is the name of the product isotope formed when Radon-222 decays by alpha decay?

katrin2010 [14]

Answer: Radon-222 is generated in the uranium series from the alpha decay of radium-226, which has a half-life of 1600 years. Radon-222 itself alpha decays to polonium-218 with a half-life of approximately 3.82 days, making it the most stable isotope of radon. Its final decay product is stable lead-20

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3 years ago

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If a compound has a composition of 82% nitrogen and 18% hydrogen, what is the empirical formula for this compound

Damm [24]

Answer: The empirical formula for the given compound is $NH_3$

Explanation : Given,

Percentage of H = 18 %

Percentage of N = 82 %

Let the mass of compound be 100 g. So, percentages given are taken as mass.

Mass of H = 18 g

Mass of N = 82 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{18g}{1g/mole}=18moles$

Moles of Nitrogen = $\frac{\text{Given mass of nitrogen}}{\text{Molar mass of nitrogen}}=\frac{82g}{14g/mole}=5.8moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 5.8 moles.

For Hydrogen = $\frac{18}{5.8}=3.10\approx 3$

For Nitrogen = $\frac{5.8}{5.8}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of H : N = 3 : 1

Hence, the empirical formula for the given compound is $NH_3$

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3 years ago

What mass of carbon monooxide must be burned to produce 175 kJ of heat under standard state condaitions?

Sphinxa [80]

Answer:

17.3124 grams

Explanation:

Given;

Amount of heat to be produced = 175 kJ

Molar mass of the carbon monoxide = 12 + 16 = 28 grams

Now,

The standard molar enthalpy of carbon monoxide = 283 kJ/mol

Thus,

To produce 175 kJ heat, number of moles of CO required will be

= Amount heat to be produced / standard molar enthalpy of CO

= 175 / 283

= 0.6183

Also,

number of moles = Mass / Molar mass

therefore,

0.6183 = Mass / 28

Mass of the CO required = 0.6183 × 28 = 17.3124 grams

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4 years ago