atio used for the conversion. TiBr4 (9) + H₂(g) → Ti(s) + HBr(g) g Ti g HBr or the following unbalanced equation, calculate how many grams of each product would be produced by complete reaction of 85.2 g of SiH4. Indicate clearly the nole ratio used for the conversion. SiH4 (9) + NH3(g) → Si3 N4 (s) + H₂(g) g Si3 N4 g H₂ or the following unbalanced equation, calculate how many grams of each product would be produced by complete reaction of 51.5 g of H₂. Indicate clearly the mole atio used for the conversion. NO(g) + H₂(g) →→ N₂ (9) + H₂O(l) g N₂ g H₂O

An alloy is found to be 41.8% Zn and the rest is Cu. If 15.0 g of Cu is added to 45.0 g of This alloy , what will be the new percentage of Cu in the alloy ?

Use 1 decimal point for all atomic masses. 82.1 g of Ni3C(s) are reacted with 1.80 g of H2(g) by the following reaction   Ni3C(s) + 2H2(g) --> 3Ni(s) + CH4(g) What is the limiting reagent? H2(g)Ni3C(s)     Based on the limiting reagent, what should the yield of Ni be?   g

What is the mass in grams of H₂ that can be formed from 40.2 grams of NH3 in the following reaction? 2 NH3(g) → 3 H₂(g) + N₂(g)

A sample of 49.0 g of tetraphosphorous decoxide (P,O10) reacts with 49.0 g of water to produce phosphoric acid (H, PO,) according to the following balanced equation. P,010 + 6 H,O → 4H,PO, Determine the limiting reactant for the reaction. H,PO, O H,0 O P,O10 Calculate the mass of H, PO, produced in the reaction. mass of H, PO4: Calculate the percent yield of H, PO, if 37.5 g of H, PO, is isolated after carrying out the reaction. percent yield:

A sample of a substance (containing only C, H, and N) is burned in oxygen.3.382 g of CO2, 2.307×10-1 g of H2O and 7.685×10-1 g of NO are the sole products of combustion.What is the empirical formula of the compound?

What is the mass in grams of H2 that can be formed from 89.6 grams of NH3 in the following reaction? 2 NH3(g) → 3 H2(g) + N2(g) 1 2 4 6. 7 8. 9. +/- х 100

Consider the following unbalanced chemical equation: Fe3O4 (aq) + CO (g) → CO2 (g) + Fe (s) What will be the coefficient in front of CO in the balanced chemical equation? If there is no coefficient in front of CO in the balanced equation, enter 1 as the answer.

[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.

Each step in the following process has a yield of 80.0%.CH4+4Cl2⟶CCl4+4HClCCl4+2HF⟶CCl2F2+2HClThe CCl4 formed in the first step is used as a reactant in the second step. If 2.00 mol CH4 reacts, what is the total amount of HCl produced? Assume that Cl2 and HF are present in excess.