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2 years ago

What are the steps to naming simple ionic compounds

2 answers:

8 0

To name an ionic compound, you simply need to find the names of the cation and anion present in the compound and make sure to revise the ends of metal names as needed. First, write out the name of the metal, followed by the name of the non-metal with its new ending.

Olegator [25]2 years ago

3 0

Answer:

Explanation:

Write the name of the cation, and then write the name of the anion, changing the ending to "-ide" if it's a single element and leaving it as it is if it's a polyatomic ion.

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If energy was added to solid, what state would it change to

12345 [234]

Answer:

Explanation:

The answer is C Liquid

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2 years ago

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How do you make a 3M solution of KBr? How many moles of KBr are 1 liter of a 0.3M solution?

pashok25 [27]

Molarity= moles/liter, so you would need 3mol KBr/1 liter
(0.3M)(1L)= 0.3mol KBr

8 0

2 years ago

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Which is the limiting reagent in the following reaction given that you start with 15.5 g of Na2S and 12.1 g CuSO4? Reaction: Na2

NemiM [27]

Answer:

CuSO4

Explanation:

Na2S + CuSO4 → Na2SO4 + CuS

The reaction is balanced (same number of elements in each side)

To determine limiting reagent you need to know the moles you have of each.

Molar mass Na2S = 23 * 2 + 32 = 78

Molar mass CuSO4 = 63.5 + 32 + 16 * 4 = 159.5

Na2S mole = 15.5 / 78 = 0.2

CuSO4 mole = 12.1/159.5 = 0.076

*Remember mole = mass / MM

With that information now you have to divide each moles by its respective stoichiometric coefficient

Na2S stoichiometric coefficient : 1

Na2S : 0.2 / 1 = 0.2

CuSO4 stoichiometric coefficient: 1

CuSO4: 0.076 / 1 = 0.076

The smaller number between them its the limiting reagent, CuSO4

8 0

3 years ago

Consider the following equilibrium: CO2(g) + C(graphite) 2CO(g); ΔH = 172.5 kJ The equilibrium constant for this reaction will

bezimeni [28]

Answer: Option (B) is the correct answer.

Explanation:

As the given reaction is as follows.

$CO_{2}(g) + C(graphite) \rightarrow 2CO(g)$

Equilibrium constant for this reaction will be as follows.

$K_{c} = \frac{[CO_{2}]}{[CO]^{2}}$

According to Le Chatelier's principle, when we increase the temperature then the equilibrium will shift towards the right hand side.

As a result, concentration of carbon dioxide will decrease whereas concentration of carbon monoxide will increase.

Thus, we can conclude that in the given reaction equilibrium constant for this reaction will decrease with increasing temperature.

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3 years ago

What is the volume of 80.0 g of ether if the density is 0.70 g/ml

My name is Ann [436]

I need to find the x pls help and show work 73838

6 0

2 years ago