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How many moles of nitric oxide NO can be produced from the decomposition of 4 moles of N2O2Cl2?
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
What else can I help you with?
A gas mixture contains 26.3 grams of nitric oxide and 36.2 grams of oxygen gas What is the mole frraction of nitric oxide?
To find the mole fraction of nitric oxide, first calculate the moles of nitric oxide and oxygen gas separately by dividing the given mass by their respective molar masses. Then, find the total moles of both gases present in the mixture. Finally, divide the moles of nitric oxide by the total moles to calculate its mole fraction.
How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide?
Using the balanced chemical equation for the decomposition of sodium azide, 2NaN3 -> 2Na + 3N2, we can see that 2 moles of Na3N produce 3 moles of N2. Therefore, for 2.88 mol of NaN3, we would produce 2.88 mol * (3 mol N2 / 2 mol NaN3) = 4.32 moles of N2.
How many moles of potassium chlorate must be used to produce 6 moles of oxygen gas?
2KClO3 --> 2KCl + 3O2For every 3 moles of oxygen gas produced, 2 moles of potassium chlorate are used.6 moles O2 * (2 moles KClO3 reacted / 3 moles O2 produced) = 4 moles KClO3
How many moles of sodium oxide will be produced when 10 moles of sodium react with oxygen This is the formula for the reaction?
Balanced equation. 4Na + O2 -> 2Na2O 10 moles Na (2 moles Na2O/4 moles Na) = 5.0 moles Na2O produced
What if a 50.0 mL o a 0.500 M solution of H2O2 is decomposed what mass of O2 will be produced?
The chemical equation for the decomposition of H2O2 is 2 H2O2 -> 2 H2O + O2. This shows that two moles of H2O2 are required to produce each mole of O2. By definition, a 0.500 M solution of H2O2 contains 0.500 moles of H2O2 in each liter of solution. Solutions are always homogeneous; therefore, 50,0 mL of such a solution will contain (0.500)(50.0/1000) or 0.0250 moles of H2O2. As noted in the first paragraph, this will produce half as many, or 0.0125, moles of O2. The gram molar mass of O2 is twice the gram atomic mass of oxygen, or 31.9988. Therefore, decomposition of this amount of H2O2 will produce 31.9988 X 0.0125 or 0.400 gram of O2, to the justified number of significant digits.
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.
How many moles of magnesium nitrate are produced when magnesium reacts with 8 moles of nitric acid?
Mg2+(s) + 2HNO3(l)= Mg(NO3)2(aq) + H2(g) since the only mole value given is 8 I must assume this is the limiting reactant. Because of the 2:1 ratio of Nitric acid to Magnesium Nitrate, meaning there must be 2 moles Nitric acid for every 1 mole Magnesium Nitrate formed, 4 moles of Magnesium nitrate will be formed.
How many moles of N2 are produced by the decomposition of 1.20 mol of NaN3?
The number of atoms is 45,166.10e23.
How many moles of no2 will be obtained starting with 0.4 moles of nitric acid?
Starting with the formula: 2HNO3 --> H2O + NO2 If you have 0.4 moles of nitric acid (HNO3), you will get half the number of moles of NO2. So, you will have 0.2 moles of nitric acid.
How many moles of NO2 will be obtained strating with 0.4 moles of nitric acid?
Starting with the formula: 2HNO3 --> H2O + NO2 If you have 0.4 moles of nitric acid (HNO3), you will end up with half the moles of nitrogen dioxide (NO2)...so you will have 0.2 moles.
What volume of nitrous oxide can be produced from the decomposition of 0.55 moles of ammonium nitrate?
Using the balanced chemical equation for the decomposition of ammonium nitrate, 2NH4NO3 --> 2N2O + O2 + 4H2O, we can see that 2 moles of nitrous oxide (N2O) is produced for every 2 moles of ammonium nitrate (NH4NO3). Therefore, 0.55 moles of NH4NO3 will produce 0.55 moles of N2O. The volume of N2O can then be calculated using the ideal gas law equation (V = nRT/P) and given conditions.
How many moles of sodium hydroxide are required to neutralize 20 mol of nitric acid?
The balanced chemical equation for the neutralization between sodium hydroxide (NaOH) and nitric acid (HNO3) is 1 mol of NaOH reacts with 1 mol of HNO3. Therefore, 20 moles of nitric acid would require 20 moles of sodium hydroxide to neutralize it.
How many moles of potassium hydroxide are needed to neutralize 3 moles of nitric acid?
The balanced chemical equation for the reaction between potassium hydroxide (KOH) and nitric acid (HNO3) is 1:1 ratio. Therefore, 3 moles of nitric acid will require 3 moles of potassium hydroxide to neutralize it.
What is the molarity of a solution of nitric acid if 0.216 g of barium hydroxide is required to neutralize 20.00 ml of nitric acid?
To calculate the molarity of nitric acid, you need to determine the number of moles of barium hydroxide used in the neutralization reaction. From there, you can use the balanced chemical equation to find the moles of nitric acid present in the solution. Finally, divide the moles of nitric acid by the volume of the solution in liters to find the molarity.
How many grams are in 2 moles of nitric acid?
1+7+(8x3) =32 =32x2 (2 moles) =64
How many moles of carbon atoms can be obtained from the decomposition of C6H6 in a 1.68 moles sample?
Each molecule of C6H6 contains 6 carbon atoms, so when 1 mole of C6H6 decomposes, 6 moles of carbon atoms are obtained. Therefore, in a 1.68 mole sample of C6H6, 6 × 1.68 = 10.08 moles of carbon atoms can be obtained from the decomposition.
