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Answer: FeCl5 Step-by-step explanation: Calculate the moles of iron and chlori...

Answer:FeCl4​ Step-by-step explanation: Moles of iron =mass of ironmolar mass ...

adaxia0226

<div style="font-family:'Helvetica Neue', Helvetica, Arial;color:#333333;"> <div> <br> <picture><source srcset="https://prealliance-textbook-qa.oneclass.com/qa_images/homework_help/question/qa_images/113/11397740.jpeg" type="image/webp"></source><img src="https://prealliance-textbook-qa.oneclass.com/qa_images/homework_help/question/qa_images/113/11397740.jpeg" alt=""></picture> </div> </div> <div id="gch" class="hidden">A 17.11 gram sample of iron is heated in the presence of excess chlorine. A metal chloride is formed with a mass of 49.73 g. Determine the empirical formula of the metal chloride. Enter the elements in the order Fe, Cl</div>

<p>A <strong class="owl-alg-value">27.67 </strong>gram sample of <strong class="owl-alg-value">iron </strong>is heated in the presence of excess <strong class="owl-alg-value">chlorine</strong>. A metal <strong class="owl-alg-value">chloride </strong>is formed with a mass of <strong class="owl-alg-value">62.79 </strong>g. Determine the empirical formula of the metal <strong class="owl-alg-value">chloride</strong>.</p>

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