chemistry

Nitric acid, a very important industrial chemical, is made by dissolving the gas nitrogen dioxide (NO2) in water. Calculate the moles of gas produced in 2 L volume container, 736 torr and 50 ºC if the gas behaves as ideal

  1. 👍
  2. 👎
  3. 👁
  1. Well the formula you need is (P x V) / T. This means pressure times volume divided by temperature. But, you need to convert your temperature to Kelvins. To do this, simply add 273 to your Celsius. Also, you need to convert torr to atmospheres. 760 torr = 1 atm. So you would have to do have 736/760. Once you do this you will have .9684211 x 2 / 323. This will give you .006 if you round up. However, you MAY OR MAY NOT still need to convert this to moles. If you do, find the molar mass and... well, I'll let you figure that out. This should give you your final answer.

    1. 👍
    2. 👎
  2. You don't write an equation. The best I can find is that 2NO2 + H2O ==> HNO3 + HNO2; i.e., a mixture of nitric and nitrous acids. And your problem asks for moles of "gas" produced in 2L ...... BUT HNO3 is not a gas. Please clarify the problem and repost. It may be that you only want the mols of NO2 gas under those conditions in which case PV = nRT and solve for n.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Write a balanced chemical equation for nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas

  2. Chemistry Balancing Equations

    Can you please tell me if these are correct? 1. Sodium Hydrogen Sulfite reacts with hydrochloric acid to produce sulfur dioxide gas, water and sodium chloride NaHSO3 + HCl -----> SO2 + H2O + NaCl 2. Sodium nitrate reacts with

  3. 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

  4. Chemistry

    The reaction between nitric oxide (NO) and oxygen to form nitrogen dioxide (NO2) is a key step in photochemical smog formation. 2 NO(g) + O2(g) 2 NO2(g) (a) How many moles of NO2 are formed by the complete reaction of 0.404 mole

  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. Chemisry

    Write a balanced equation using the correct formulas and include conditions (s,l,g or aq) for each of the following reactions. 1)Carbon monoxide gas reacts oxygen gas to produce carbon dioxide gas. Express your answer as a

  3. 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

  4. chemistry

    Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 23°C and 0.94 atm, the density of this gas mixture is 2.6 g/L. What is the partial pressure of each gas?

  1. 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

  2. Chemistry

    give the balanced equation for: Liquid nitric acid decomposes to reddish brown nitrogen dioxide gas, liquid water, and oxygen gas. the equation i got was HNO3 --> NO2+ H2O+ O2 is that right? i haven't balanced it yet

  3. Chemistry PLS HELP

    The cover plate is removed from the gas jars shown iin the diagram. Nitrogen dioxide is a brown gas. After several days, the color of the gas is the same in both of the jars. What explains this change? So the picture shows this

  4. Chemistry

    Deduce the number of nitrogen atoms in: 5.00 x 10^-3 mol of ammonia, NH3 and 4.601 g of nitrogen dioxide, NO2

You can view more similar questions or ask a new question.