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A student is trying to figure out how many moles of potassium chloride are formed from 4.0 grams of chlorine gas. Which step in the following students work is incorrect?

A student is trying to figure out how many moles of potassium chloride are formed-example-1

1 Answer

5 votes

Answer:

Step 3 ⇒ incorrect

Further explanation:

Given

mass of Cl₂ : 4 g

Required

incorrect step

Analysis

analyze step

  • balanced equation
  • determine mol of Cl₂
  • mol ratio from equation
  • potassium chloride formed

Solution

  • balanced equation

Reaction

2K(s)+Cl₂(g)⇒2KCl(s)

Step 1⇒correct

  • determine mol of Cl₂

we determine the moles of Cl₂ by their mass

MW of Cl₂=70.9 g/mol

mol=mass : MW

Step 2 ⇒ correct

  • mol ratio from equation

From equation, mol ratio of Cl₂ to KCl = 1 : 2, so mol KCl :


\tt mol~KCl=(2)/(1)* 0.0564=0.1128

Step 3 ⇒ incorrect

Paraphrase

Step 3 ⇒ incorrect

User Simon Brangwin
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