if 11.6 grams of O3 reacts with excess NO, how many g of NO 2 will be produced? ___ g NO2

Consider the following unbalanced chemical equation: C+ O2 -> CO2. Given 2 moles of carbon, how many moles of oxygen are needed to burn out the carbon?

N2 + 3H2 → 2NH3 How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen? O 10.8 g H2 O 11 g H2 O 13 g H2 O 9.8 g H2

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Complete combustion of a 1.448 g sample of a hydrocarbon (only carbon and hydrogen present), produced 3.128 g of CO₂ and 1.121 g of H₂O What is the empirical formula of the compound? O C4H7 O CH2 O C₂H7 O C₂H5 O C3H8

___O2 + ___Fe  --->   ___Fe2O3 a. How many moles of oxygen will produce 6.2 moles of iron (III) oxide?  b. How many moles of iron (III) oxide could be produced if 3.25 moles of O2 are reacted? c. How many moles of Fe are required to produce .33 moles of iron (lll) oxide?

What mass of hydrogen peroxide (H2O2) must decompose to produce 65.88 g of H2O?

2 N2O5 ----> 4 NO2  +  O2 What mass of NO2 can be produced from the complete reaction of 38.2 g of N2O5?

This is one question with four different parts. Please answer all four parts. Thank you

When the equation for the combustion of ethanol (C2H5OH) is balanced with lowest whole number coefficients, the coefficient in front of oxygen is? A) 3 B 14 7