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Nadusha1986 [10]
2 years ago
8

The element nickel has five naturally occurring isotopes. Which of the following describes the relationship of these isotopes?

Chemistry
1 answer:
Elden [556K]2 years ago
6 0
<h3>Answer:</h3>

Different mass, same atomic number

<h3>Explanation:</h3>
  • Elements are made of similar atoms, however the atoms may have different number of neutrons but the same number of protons in their nucleus.
  • Such atoms that have equal number of protons but different number of neutrons are known as isotopes.
  • Difference in the number of neutrons makes isotopes to have different mass numbers.
  • Atomic number is the number of protons in the nucleus of an atom, therefore, isotopes have the same atomic number.
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When comparing the colors of the following four compounds, which is most likely to appear green? [Co(CN)6]3− [Co(H2O)6]3+ [Co(en
alexandr1967 [171]

Answer:

3

Explanation:

its bc

5 0
3 years ago
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Comment Both propane and benzene are hydrocarbons. As a rule,
kozerog [31]

The enthalpy change : -196.2 kJ/mol

<h3>Further explanation  </h3>

The change in enthalpy in the formation of 1 mole of the elements is called enthalpy of formation  

The enthalpy of formation measured in standard conditions (25 ° C, 1 atm) is called the standard enthalpy of formation (ΔHf °)  

(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)  

The value of ° H ° can be calculated from the change in enthalpy of standard formation:  

∆H ° rxn = ∑n ∆Hf ° (product) - ∑n ∆Hf ° (reactants)  

Reaction

2 H₂O₂(l)-→ 2 H₂O(l) + O₂(g)

∆H ° rxn = 2. ∆Hf ° H₂O - 2. ∆Hf °H₂O₂

\tt \Delta H_{rxn}=2.(-285.8)-2.(-187.8)\\\\\Delta H_{rxn}=-571.6+375.4=-196.2~kJ/mol\rightarrow \Delta Hf~O_2=0

5 0
3 years ago
A compound of mercury and oxygen is heated in order to decompose the compound. A 4.08 grams sample of mercury oxide upon heating
arlik [135]

Answer:

HgO (empirical formula)

Explanation:

4.08 - 3.78 = 0.3g (oxygen)

(\frac{4.08}{201})   \:  \:  \:  (\frac{0.3}{16} )

0.02 : 0.02

0.02/0.02 : 0.02/0.02

1 : 1 (ratio)

HgO ( empirical formula)

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7 0
2 years ago
what is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g​
LekaFEV [45]

Answer:

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Explanation:

Find the molar mass of K2SO4 first:

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Divide the goal molar mass of 696 by the molar mass of the empirical formula:

696 / 174 = 4

This means you need to multiply everything in the empirical formula by 4:

K2SO4 --> K8S4O16 or K8(SO4)4 depending on if the SO4 is for sulfate or not

4 0
2 years ago
In a chemical reaction, the reactants (beginning elements or compounds) but have the same number and type of atoms as the produc
AleksAgata [21]

Answer:The law of conservation of matter says that matter cannot be created or destroyed. In chemical equations, the number of atoms of each element in the reactants must be the same as the number of atoms of each element in the products. ... There are two oxygen atoms in the reactants and two atoms of oxygen in the product.

Explanation:

4 0
3 years ago
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