chem 1 high school

equation: 4NH3(g) + 5O2(g) -> 4NO(g) + 6H2O(g)
What mass of O2 is needed to produce 0.563g of NO? I think the answer is 750g but how do I get that answer?

  1. 👍 0
  2. 👎 0
  3. 👁 254
  1. A stoichiometry problem. Here is a solve example. Just follow the steps.

    1. 👍 0
    2. 👎 0
  2. It certainly won't take more than 1000 times as much O2 to make that much NO. Did you omit a decimal point somewhere?

    Five moles of O2, with a mass of 160 g, are all that is required to make 4 moles of NO, with a mass of 112 g.

    Try applying the 160/112 ratio to the amount of NO you want to produce.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Industrially, nitric acid is produced by the Ostwald process represented by the following equations: 4NH3 +5O2 = 4NO +H2O 2NO +O2 = 2NO2 2NO2 +H2O = HNO3 +HNO2 What mass of NH3 (in grams) must be used to produce 1.0 ton of HNO3 by

  2. Chemistry

    4NH3+5O2 = 4NO + 6 H20 If a container were to have 10 molecules of O2 and 10 molecules of NH3, initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?

  3. Chem

    Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(g) 2NO(g) + O2(g) > 2NO2 (g) 3NO2(g) + H2O(l) > 2HNO3(aq) + NO(g) What mass of NH3 must be used

  4. Chemistry

    Calculate Delta H for 4NH3 + 5O2 --> 4NO + 6H2O using: N2 +O2 --> 2NO DH= -180.5 kJ N2 + 3H2 --> 2NH3 DH= -91.8 kJ 2H2 + O2 --> 2H2O DH= -483.6 kJ

  1. Chemistry

    Nitric acid can be produced from NH3 in three steps process: I)4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) II)2NO(g) + O2(g) → 2NO2(g) III)3NO2(g) + H2O(l) →2HNO3(aq) + NO(g) % yield of Ist, IInd & IIIrd are respectively 50 % , 60 %

  2. stoichiometry

    Ammonia gas reacts with oxygen gas according to the following equation: 4NH3 + 5O2----4NO + 6H2O a. How many moles of oxygen gas are needed to react with 23 moles of ammonia? (29 mole) b. How may grams of NO are produced when 25

  3. chemistry

    4NH3 + 5O2 → 4NO + 6H2O 2NO + O2 → 2NO2 3NO2 + H2O → 2HNO3 + NO In this process, the NO made in the last reaction is recycled back into the second reaction and used as a reactant. In the end, all of the NO produced is

  4. Chemistry

    Consider the following reaction: 4NH3(g) +5O2(g) -->4NO(g) +6H2O(g) Suppose we have two flasks connected by a stopcock. In one flask, we have 2.0L of NH3(g) at a pressure of .500 atm. In the other flask, we have 1.00L of O2(g) at

  1. chemistry

    4NH3(g)+5O2(g) yield 4NO(g)+6H2O(g) Deduce the equilibrium constant expression for the reaction.

  2. chemistry

    In which reaction does the smallest percentage change in volume occur? a) C3H8 (g) + 5O2(g) ---> 3CO2(g) + 4H2O(l) b) 4NH3(g) + 3O2(g) ----> 2N2(g) + 6H2O(l) c) CH4(g)+ 2O2(g) ----> CO2(g) + 2H2O(l) d) 2H2S(g) + SO2 (g) ---->

  3. Chemistry

    Consider the following equation: 4NH3(g) + 5O2(g)----> 4NO(g)+6H2O(g) a. How many liters of oxygen are required to react with 2.5 L NH3? Both gases are at STP b. How many grams of water vapor can be produced from 25 L NH3 if both

  4. Chemistry

    for the reaction 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g) if H = -950kJmol-1, does that mean it's an exothermic reaction? Ooops pressed Post too quickly. Yes it is exothermic. Delta H is negative so heat is lost from the system. If delta

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