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vfiekz [6]
3 years ago
5

Which of these pairs would form an ionic bond? K and Br

Chemistry
2 answers:
weeeeeb [17]3 years ago
8 0

Answer:

K and Br

Explanation:

I got it right duhhh

ZanzabumX [31]3 years ago
5 0

is there any other pairs


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How mamy moles of NaCl will be produced from 83.0g of Na, assuming Cl2 is available in excess
Anestetic [448]

Answer:

3.62moles

Explanation:

First let us generate a balanced equation for the reaction

2Na + Cl2 —> 2NaCl

Molar Mass of Na = 23g/mol

Mass of Na from the balanced equation = 2 x 23 = 46g

Molar Mass of NaCl = 23 + 35.5 = 58.5g/mol

Mass of NaCl from the balanced equation = 2 x 58.5 = 117g

From the question,

46g of Na produced 117g of NaCl.

Therefore, 83g of Na will produce = (83 x 117)/46 = 211.11g of NaCl

Converting this mass (211.11g of NaCl) to mole, we obtain:

n = Mass /Molar Mass

n = 211.11/ 58.5

3.62moles

8 0
3 years ago
Determine the pHpH of an HFHF solution of each of the following concentrations. In which cases can you not make the simplifying
PIT_PIT [208]

The question is incomplete, complete question is :

Determine the pH of an HF solution of each of the following concentrations. In which cases can you not make the simplifying assumption that x is small? (K_a for HF is 6.8\times 10^{-4}.)

[HF] = 0.280 M

Express your answer to two decimal places.

Answer:

The pH of an 0.280 M HF solution is 1.87.

Explanation:3

Initial concentration if HF = c = 0.280 M

Dissociation constant of the HF = K_a=6.8\times 10^{-4}

HF\rightleftharpoons H^++F^-

Initially

c          0            0

At equilibrium :

(c-x)      x             x

The expression of disassociation constant is given as:

K_a=\frac{[H^+][F^-]}{[HF]}

K_a=\frac{x\times x}{(c-x)}

6.8\times 10^{-4}=\frac{x^2}{(0.280 M-x)}

Solving for x, we get:

x = 0.01346 M

So, the concentration of hydrogen ion at equilibrium is :

[H^+]=x=0.01346 M

The pH of the solution is ;

pH=-\log[H^+]=-\log[0.01346 M]=1.87

The pH of an 0.280 M HF solution is 1.87.

6 0
2 years ago
Explain why energy sources do not have 100% efficiency. Why do you think some have lower efficiencies?
bearhunter [10]

Answer:

Energy sources do not have 100% efficiency because <em>the processes of energy conversion to usable forms involves energy losses. </em>

Some have lower efficiencies due to; <u>energy losses in form of heat</u> during conversion, <u>poor technology applied during conversion</u> of energy and<u> lack of desire equipment</u> to use in the energy conversion system.

Explanation:

The desired form of energy for use is derived from conversion of energy from the source using an energy converter into another form which is usable. The efficiency of the energy converter is calculated as;

л = output energy/input energy

The efficiency of energy is limited to the cost of equipment required for conversion from energy source by the energy converter to a form which is usable. Additionally, because energy sources are scarce, the technology to use in energy  conversion is a factor affecting energy efficiency in that high efficiency will require advanced technology with better equipment leading higher costs of that energy form. when heat losses are involved during energy conversion, efficiency lowers, thus its better if such losses are used as energy input in another system.

5 0
3 years ago
The change in enthalpy is the change in heat energy of a reaction and is calculated by (Hint: Hess' Law): Group of answer choice
Stolb23 [73]

Answer:

d. Sum of product enthalpies minus the sum of reactant enthalpies

Explanation:

The standard enthalpy change of a reaction (ΔH°rxn) can be calculated using the following expression:

ΔH°rxn = ∑n(products) × ΔH°f(products) - ∑n(reactants) × ΔH°f(reactants)

where,

ni are the moles of products and reactants

ΔH°f(i) are the standard enthalpies of formation of products and reactants

8 0
3 years ago
2,3-Dimethylbutane reacts with bromine in the presence of light to give a monobrominated product. Further reaction gives a good
irga5000 [103]

Answer:

Explanation:

find the solution below

3 0
3 years ago
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