Note: Use the Smaller Amount of Product (SAP) approach for this problem. All remaining conversion steps begin with the SAP amount.Octane (C8H18, MM = 114.23 g/mol) is a component of gasoline. Combustion of octane is represented by the following balanced chemical equation2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)If a reaction mixture contains 218 g C8H18 and 455 g O2, (a) Identify the limiting reactant and excess reactant based on the SAP math. [4 points](b) How many grams of CO2 are expected to form? [1 point](c) How many moles of H2O are expected to form? [2 points](d) How many grams of excess reactant are consumed in the reaction? [2 points](e) How many grams of excess reactant are left over once the reaction is complete? [1 point]Enter the following in the text box provided and show your full work on scratch paper.(a) Limiting reactant = _____________ (type the chemical formula) and excess reactant = _____________ (type the chemical formula).(b) Mass of CO2 = ______________ g CO2. Enter the value in the text box.(c) Moles of H2O expected to form = ______________ mol H2O. Enter the value in the text box.(d) Mass of excess reagent consumed in the reaction = ______________ g. Enter the value in the text box.(e) Mass of excess reagent left over after the reaction is complete = ______________ g. Enter the value in the text box.

Consider a redox reaction: Mg + Cu2+ → Mg2+ + Cu. Which of the following is/are true? Select all that apply.(Hint: OIL RIG)(A) Mg is reduced.(B) Cu2+ is reduced.(C) Mg is oxidized.(D) Mg is oxidized.

The balanced equation for the combination reaction of hydrogen gas and solid iodine is: H2(g) + I2(s) + 52 kJ → 2 HI(g) Is this reaction is exothermic or endothermic? [BLANK-1]. The enthalpy change (∆H) value for this reaction should be indicated with positive or negative sign. [BLANK-2].

What coefficient is placed in front of O2 to complete the balancing of the following equation?  CH4(l) + ? O2(g) → CO2(g) + 2 H2O(g)

Consider a hypothetical compound with the chemical formula: C15H14O11. The molar mass of this compound is _________ g/mol.Note: Make sure to use the atomic masses given in the periodic table provided. Round the final answer to 5 significant figures.

If the electronegativity difference between the bonded atoms is 2.0 or higher, the bond is considered _____________.

Consider three samples of sodium compounds:1 mol Na2SO4, 1 mol Na2CO3, and 1 Na2HPO4 All three samples have same number of sodium atoms.

The calculations show that a reaction should produce [x] g of the product. However, a chemistry lab experiment produces [y] g of pure product. What is the percent yield of this product? ____________%. Just enter the number (without percent symbol).

Consider the following reaction: 2 KClO3(s) →∆ 2 KCl(s) + 3 O2(g)What type of reaction is this?

Consider a chemical compound with the empirical formula CxHyOz. The mass percent data for this compound is summarized below:C = 17.03%, H = 3.57% and O = 79.40% by mass. Determine the empirical formula for this compound. Make sure to keep at least 4 decimal places in your mole calculations and enter the empirical formula in CxHyOz format (x, y, z = whole numbers). Do not change the order of elements. Enter the empirical formula in the text box provided and show complete work on the scratch paper. You must submit your work to receive credit. [Hint: Use the Percent → Grams → Mol → Simplest Whole Number sequence.]