chemistry

a) Calculate the number of moles of nitrogen dioxide, NO2, that could be prepared from 79.0 mol of nitrogen oxide and 82.0 mol of oxygen.

2NO(g)+O2(g)⟶ 2NO2(g)

b) Identify the limiting reagent and the excess reagent in the reaction. What would happen to the potential yield of NO2 if the amount of NO were increased?

c) What if the amount of O2 were increased?

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
  1. for every mole of O2, one needs 2 moles NO, and gets 2 mole of NO2

    82 moles of O2 would require 164 mole NO, which is not there.
    So NO is the limiting reactant.
    79 moles NO>>>>79 moles NO2
    Adding more NO>>>>making more NO2
    adding more O2, no effect.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    👤
    bobpursley
  2. Thank you!

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩

Respond to this Question

First Name

Your Response

Similar Questions

  1. General Chem

    Nitrogen oxide reacts with oxygen gas to form nitrogen dioxide (NO2). In one experiment 0.866 mole of NO is mixed with 0.503 mole of O2. Calculate the number of moles of NO2 produced

  2. chemistry

    Copper(II) nitrate decomposes upon heating to form copper(II) oxide, nitrogen dioxide gas, and oxygen gas. If 1.0 mole of copper(II) nitrate decomposes, how many moles of nitrogen dioxide would be formed?

  3. Chemistry

    A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O3(g)+NO(g) --> O2(g)+NO2(g) The rate law for this reaction is: rate=k[O3][NO] Given that k = 2.87 × 106 M–1·s–1 at a

  4. science

    from the balanced equation 4NH3 +7O2 - 4NO2 + 6H2O. How many grams of oxygen are necessary to produce 4.50 moles of NO2? I think its 11 grams or 22 grams but im not sure. please help!! First the number of moles of O2, molesO2=

  1. Chemistry

    Nitrogen Dioxide NO2 decomposes upon heating to form nitric oxide and oxygen according to the following equation: 2NO2(g) --> 2NO(g) + O2(g) At the beginning of an experiment the concentration of nitrogen dioxide in a reaction

  2. Chemistry

    Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2 (g)+ H2O (l) --> 2HNO3 (l) + NO (g) Suppose that 5 mol NO2 and 1 mol H2O combine and react completely. How many moles of

  3. AP chemistry

    The mechanism for the reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be NO2+NO2 > NO3+NO slow NO3+CO > NO2+CO2 fast Write the rate law expected for this mechanism. What is

  4. chemistry

    how do i solve the following problem? Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300°C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of

  1. chemistry

    In the formation of smog, nitrogen and oxygen gas react to form nitrogen dioxide: N2(g)+2O2(g)→2NO2(g)How many grams of NO2 will be produced when 2.1L of nitrogen at 840mmHg and 28∘C are completely reacted? I know that you use

  2. Calculus

    4. At high temperatures, nitrogen dioxide, NO2, decomposes into NO and O2. If y(t) is the concentration of NO2 (in moles per liter), then at 600 degrees K, y(t) changes according to the reaction law dy/dt = −. 05y2 for time t in

  3. chemistry

    In the reaction O2+2NO->2NO2 what is the ratio of oxygen reacted to nitrogen dioxide produced? Nitrogen monoxide to nitrogen dioxide? We had to calculate the concentration of each, for which I have O2=-1.01x10^-5, NO=-2.03x10^-5

  4. physics

    A 22.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.40 105 Pa and temperature of 22.0°C. (a) Calculate the temperature of the gas in Kelvin. K (b) Use the ideal gas law to calculate the number of moles of gas in the

View more similar questions or ask a new question.