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Which of the following equations is balanced correctly and has the correct products for the reactants RbNO3 and BeF2?3RbNO3 + 3BeF2 → Be(NO3)3 + 3RbF, because Be increases in charge from 2+ to 3+ when it is replaced2RbNO3 + BeF2 → Be(NO3)2 + 2RbF, because Be keeps a 2+ charge throughout the reactionRbNO3 + BeF2 → BeNO3 + RbF2, because Be keeps a 1+ charge throughout the reaction2RbNO3 + BeF2 → Be(NO3)2 + 2RbF, because Be increases in charge from 1+ to 2+ when it is replaced

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superman1987

Answer:

2RbNO₃ + BeF₂ → Be(NO₃)₂ + 2RbF, because Be keeps a 2+ charge throughout the reaction.

Explanation:

  • It is a double replacement reaction.
  • A double replacement reaction is a type of chemical reaction where two compounds react, and the positive ions (cation) and the negative ions (anion) of the two reactants switch places, forming two new compounds or products.
  • In this reaction, there is no change in the oxidation state of different atoms.
  • It is just a replacement reaction.

  • So, the right choice is:

2RbNO₃ + BeF₂ → Be(NO₃)₂ + 2RbF, because Be keeps a 2+ charge throughout the reaction.

realparisbaron

Answer:

b

Explanation:

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