Consider the reaction given below and answer the succeeding questions. Express all answers in proper significant figures. 3 TiO2(s) + 4 C(s) + 6 Cl2(g) → 3 TiCl4(g) + 2 CO2(9) + 2 CO(g) Molar masses (MM): TiO2(s) = 79.87; C(s) = 12.01; Cl2(g) = 70.91; TiCl4(g) = 189.68; CO2(g) = 44.01; CO(g) = 28.01. 1. What mass of TiCl4 is produced by reacting 100.0 g TiO2, 100.0 g Cl2, and 100.0 g of C? g 2. How much of the reactant/s is/are left? g TiO2, g C(s), g Cl2

Sodium carbonate, Na2CO3, is commonly used to neutralize acid spills in the laboratory. The neutralization of nitric acid is described by the UNBALANCED chemical equation HNO3 + Na2CO3 ➜ CO­2 (g) + H2O + NaNO3 How much Na2CO3 (molar mass: 105.99 g/mol) is required to neutralize 1.50 × 102 g of spilled nitric acid (molar mass: 63.01 g/mol)?   a.252 g Na2CO3 b.126 g Na2CO3 c.505 g Na2CO3 d.150 g Na2CO3

The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). What is the mass in grams of phosphorus trichloride that can be formed from 226.0 grams of chlorine gas based on the balanced chemical equation?

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. [] → Ba(C1O₂)₂(aq) + H₂O(1) 2 X G

The complete combustion of gasoline (C8H18) is best represented by which of the following equations:   2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O(l)   2 C8H18 (l) + 17 O2 (g)  → 16 CO (g) + 9 H2O (l)   C8H18 (l)  → 8 C (s) + 9 H2 (g)   C8H18 (l) + O2(g) → 8 CO2 (g) + 9 H2O (l)   C8H18 (l) + O(g) → 8 CO2 (g) + 9 H2O (l)

In an experiment, zinc chlorate decomposed according to the following chemical equation.Zn(ClO3)2 → ZnCl2 + O2(Molar mass of Zn(ClO3)2 = 232.29 g/mol; ZnCl2 = 136.286 g/mol; O2 = 31.998 g/mol)If the mass of zinc chlorate was 150 grams, which of the following calculations can be used to determine the mass of oxygen gas formed?    (150 × 1 × 232.29) ÷ (31.998 × 3) grams  (150 × 3 × 232.29) ÷ (31.998 × 1) grams  (150 × 1 × 31.998) ÷ (232.29 × 3) grams orr (150 × 3 × 31.998) ÷ (232.29 × 1) grams

1.) What is the molar mass for aluminum sulfate? Please use the atomic masses on the periodic table. Express your answer with the correct significant figures and units for molar mass. Mass Choices:  123.05 342.17 6.02 x 10^23 273.08 Unit Choices:  mol mol/g g g/mol 2.) How many grams are there in 5.699 moles of copper, Cu?  Express your answer with the appropriate significant figures and units.  0.08968 g/mol Cu 362.2 g/mol Cu 362.2 g Cu 0.08968 g Cu

Balance the following chemical reaction. Enter the sum of the balanced coefficients as your answer. Assign "blank" coefficients a value of 1. silver iodide + sodium sulfide → silver sul fide + sodium iodide

[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.

What is the total number of oxygen atoms on the right-hand side of this chemical equation? 8 Al(s) + 3NaNO3(aq)+5NaOH(aq)+18H₂O(1) → 8 NaAl(OH)4(aq) +3NH₂(g)