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Answer: 8 mol NO

First, you start by writing the decomposition of N2O2CL2:

N2O2Cl2=> 2NO +Cl2

(in reality, we should expect NO2 or N2 and O2 to be products in place of NO, but we'll assume the problem given expects this decomposition)

Then, using stochiometry: 4 mol N2O2Cl2 * 2 mol NO/1 mol N2O2Cl2= 8 mol NO

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How many moles of sodium oxide will be produced when 10 moles of sodium react with oxygen This is the formula for the reaction?

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Related Questions

What weight of nitric acid can be produced from 18.5 gram of nitrogen dioxide?

To calculate the weight of nitric acid produced from 18.5 grams of nitrogen dioxide, you need to consider the stoichiometry of the reaction. The balanced chemical equation is: 2NO2 + H2O -> HNO3 + NO From the equation, we see that 2 moles of nitrogen dioxide produce 1 mole of nitric acid. First, convert 18.5 grams of nitrogen dioxide to moles, then use the mole ratio to find the moles of nitric acid produced. Finally, convert the moles of nitric acid to grams using the molar mass of nitric acid.


How many moles (precise to the nearest 0.01 mol) of nitric acid are produced from 300.00 mol of nitrogen dioxide?

To determine how many moles of nitric acid (HNO₃) are produced from nitrogen dioxide (NO₂), we refer to the balanced chemical equation for the formation of nitric acid from nitrogen dioxide and oxygen: [ 4 \text{NO}_2 + \text{O}_2 \rightarrow 4 \text{HNO}_3 ] From the equation, 4 moles of NO₂ produce 4 moles of HNO₃, indicating a 1:1 mole ratio. Therefore, from 300.00 moles of NO₂, 300.00 moles of HNO₃ will be produced.


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How many moles of NO2 will be obtained strating with 0.4 moles of nitric acid?

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