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What errors did the chemistry teacher make in planning to this demonstration and how could checking her work have made a difference?

*THERE ARE A TOTAL OF 4 ERRORS* NEED HELP ASAP BEFORE 11:59 PM

With the hope of sharing an explosive combustion reaction demonstration in class
for her students, a chemistry teacher decides to synthesize water. This process
occurs when oxygen gas (O₂) in the air is combined with hydrogen gas, H₂, in the
presence of a spark or small flame. Like the reactants, the water (H₂O) product is
also a gas.
She knew she didn't want the demonstration to create too much water product,
only 180.0 grams.
Since the oxygen reactant is abundantly present in the air, she needed only to
determine how much hydrogen gas to prepare before class.
She used the following chemical equation to make her predictions:
O2(g) + H2(g) → H₂O(g)

What Errors Did The Chemistry Teacher Make In Planning To This Demonstration And How Could Checking Her Work Have Made A Difference THERE ARE A TOTAL OF 4 ERROR class=

Sagot :

mickymike92

The teacher used have used standard temperature and pressure values in her calculations of volume of hydrogen gas required.

What is the equation for the synthesis of water?

The equation for the synthesis of water is given below as follows:

[tex]2 H_2 + O_2 \rightarrow 2H_2O[/tex]

Based on the planned steps of the synthesis of hydrogen gas by the teacher, the following errors were committed by the teacher:

  1. She used temperature in degrees Celsius for her calculations
  2. She used the mass of water required instead of moles of water in her calculation using the ideal gas equation
  3. She did not use standard temperature and pressure measurement in her calculations
  4. She used an unbalanced chemical equation for her calculation

Therefore, in calculation molar volume of gases, the measurements should be taken at standard temperature and pressure values.

Learn more about molar gas volume at: https://brainly.com/question/15026766

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