If possible could it be in scientific notation as it shows underneath

Balance the following chemical reaction and determine the number of moles of HI produced when 2.36E0 moles of H2(g) are consumed in the following chemical reaction: H2(g)+I2(g)_HI(g) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) Balance the following chemical equation and determine the number of moles of Fe(s) produced when 8.1E1 moles of Fe2O3(s) react with excess C(s) to produce Fe(s) and CO2 (g). Fe2O3(s)+C(s)Fe(s)+CO2(g) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) Balance the following chemical equation and determine the number of moles of CO2(g) produced when 4.051020 molecules of C6H12O6(s) react with excess O2(g) to produce CO2(g) and H2O. C6H12O6(s)+O2(g)CO2(g)+H2O(l) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) Consider the following chemical reaction: 2CH3OH(l)+3O2(g)2CO2(g)+4H2O(l) Calculate the number of moles of CO2 produced when 1.154E1 mL of methanol CH3OH(I) reacted completely with O2(g). The density of methanol is 0.79g/mL. Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) Coal power plants burn large amounts of coal, C(s), in an O2(g) atmosphere to generate electricity. The chemical reaction responsible for producing this energy is shown below: C(s)+O2(g)CO2(g) Determine the mass in grams of CO2 produced when 1.20E2 metric tons of C(s) are completely burned in an O2 atmosphere (1 metric ton =103kg= 106g). Don't include units in your answer Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) For the chemical reaction below, determine the amount of HI produced when 3.41E0g of hydrogen is reacted with 5.021E1g of iodine to produce hydrogen iodide (HI). H2(g)+I2(g)2HI(g) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) In the following chemical reaction, how many grams of the excess reactant are left over when 4.79E-1 moles of Al(s) react with 1.11E0 moles of Cl2(g) ? 2Al(s)+3Cl2(g)2AlCl3(s) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) For the following chemical reaction, determine the amount of water in grams produced when 2.0510 23 molecules of H2 react with 1.331023 molecules of O2 to produce water 2H2(g)+O2(g)2H2O(l) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 ) Using the following equation, determine the % yield from the following reaction if 3.080E1g of octane ( C 8H18 ) react with excess oxygen to produce 8.160E1 g of CO2(g). 2C8H18(l)+25O2(g)16CO2(g)+18H2O(l) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5 e5 for 2.5105 ) For the following reaction, determine the amount of AgCl(s) formed when 1.046E1g of KCl(aq) react with excess AgNO3(aq) to produce AgCl(s) and KNO3(aq) with a 7.706E1% yield. AgNO3(aq)+KCl(aq)AgCl(s)+KNO3(aq) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5e5 for 2.5105 )