This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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c) Step 1: Write the balanced chemical equation for the combustion of carbon (II) oxide. 2CO(g) + O_2(g) → 2CO_2(g) Step 2: Determine the volume ratios from the balanced equation. From the equation, 2 volumes of carbon monoxide react with 1 volume of oxygen to produce 2 volumes of carbon dioxide. Step 3: Calculate the volume of oxygen required to react with 200 cm^3 of carbon monoxide. Volume of O_2 required = (1)/(2) × Volume of CO Volume of O_2 required = (1)/(2) × 200 cm^3 = 100 cm^3 Step 4: Identify the limiting reactant and the excess reactant. Given 150 cm^3 of oxygen, and only 100 cm^3 is required, oxygen is in excess. Carbon monoxide is the limiting reactant. Step 5: Calculate the volume of remaining oxygen. Volume of O_2 remaining = Initial volume of O_2 - Volume of O_2 reacted Volume of O_2 remaining = 150 cm^3 - 100 cm^3 = 50 cm^3 Step 6: Calculate the volume of carbon dioxide produced. Volume of CO_2 produced = Volume of CO reacted (due to 2:2 ratio) Volume of CO_2 produced = 200 cm^3 The remaining gases are carbon dioxide and oxygen. The volume of carbon dioxide is 200 cm^3. The volume of oxygen is 50 cm^3. 4. (a) The patient should take 2 tablets, 3 times a day, for 3 days. 4. (b) Sample 1 registered a higher temperature, meaning Flame I is hotter. A hotter flame from a Bunsen burner is produced when the air hole is fully open, resulting in a non-luminous (blue) flame. Send me the next one 📸