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The provided balanced equation applies to the reaction that takes place between zinc metal and copper(I) nitrate.
Zn +2 CuNO3 - Zn(NO3)2 + 2 Cu
If the reaction begins with 0.037 moles of zinc and 0.11 moles of copper(I) nitrate, how many grams of copper metal can be produced? Assume 100%
yield. Round off your answer to the nearest tenth of a gram. Record your answer in the grid.

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Mass of copper produced = 5 g

The balanced chemical equation:

Zn + 2CuNO₃ → Zn(NO₃)₂ + 2Cu

Given:

0.037 moles of zinc and 0.11 moles of copper(I) nitrate

To find:

Mass of Cu  metal produced=?

The amount of CuNO₃  produced =0.11/2=0.055moles

Thus, amount of copper=0.037*2= 0.0740 moles  

The mass of copper produced =0.0740*63.5=4.699g=5g

Therefore, the Mass of Cu produced will be 5 g.

Learn more:

brainly.com/question/13852350

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