t volume is occupied by a 0.908 mol sample of neon gas at a temperature of 0 °C and a pressure of 1 atm? ubmit Answer L Retry Entire Group 4 more group attempts remaining

diagram b is correct,     What procedures can be used to solve this problem? write down the plan for this new way to solve the problem.  1. first execute plan 1 to solve this problem. explain in every step. 2. solve the problem again - this time use the plan that you propose, plan 2. 3. finally, think about the way that you can use it to make sure that your answer makes sense. write your assessment.

Not too sure if the answer is 124 g or 0.124 g.

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.

how did you get the numbers beside the balanced equations. such as 4 beside H2O and 2 beside N2.

Chemistry GAM The diagram (Figure 1) represents a high-temperature reaction between CH4 and H₂O. Figure Part A Based on this reaction, find how many moles of CO can be obtained starting with 5 mol CH₂? Express your answer as an integer. | ΑΣΦ 1 → C ? n = mol Part B Based on this reaction, how many moles of H₂ can be obtained starting with 5 mol CH4? Express your answer as an integer. IVE ΑΣΦ ? n= Submit Request Answer mol

Consider the reaction 3X + 2Y → 5C + 4D With excess Y, how many moles of X are needed to produce 13.00 moles of D?

[Review Topics] [References] "Smelling salts," which are used to revive someone who has fainted, typically contain ammonium carbonate, (NH4)2CO3. Ammonium carbonate decomposes readily to form ammonia, carbon dioxide, and water. The strong odor of the ammonia usually restores consciousness in the person who has fainted. The unbalanced equation is (NH4)2CO3 (8)→ NH3(g) + CO₂(g) + H₂O(g) Calculate the mass of ammonia gas that is produced if 0.850 g of ammonium carbonate decomposes completely. g NH3 Submit Answer Mastered Retry Entire Group 8 more group attempts remaining Previous Next Save and Exit

Which reaction has the largest AS? ON₂(g) + 3H₂(g) → 2NH3(9) □2NO(g) → N₂O2(g) O2N₂ H₁(g) →→→ 2NH3(g) + H₂(g) □ O₂(g) + 2H₂(g) → 2H₂O(g) □ O2(g) +2H₂(g) → 2H₂O(l)

Does the product formed during the combustion of magnesium in Test 6 (the ashy magnesium oxide) to weigh more than, less than, or the same as the original piece of magnesium? Explain.