chemistry help!!

a gaseous mixture contains 1 mol of O2 and 2 mol of CO2, exerting a total pressure of 1.5 atm. what amount of CH4 must be added to the mixture in order to increase the total pressure to 2 atm. (assume no gas escapes and there is no change in total volume)

the answer is 1 mol but i do not know how to get to that answer!

  1. 👍 0
  2. 👎 0
  3. 👁 243
  1. P1/n1 = P2/n2

    P1 is the original total pressure (1.5 atm), n1 is the total moles: (1 mol O2 + 2 mol CO2= 3 moles total.)

    P2 is the new total pressure (2 atm), n2 is the new total moles, which is 3 moles + x moles CH4 added.

    1.5/3 = 2/ (3+x)

    solve for x
    x= moles CH4 added= 1 mol

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemsitry

    The equilibrium between three substances, a, B and c is shown below. A(g) + B(g) C(g) Initially there were 0.1 mol of a and 0.2 mol of B in the reaction mixture. a and B reacted together to produce an equilibrium mixture

  2. Chemistry

    Which of the reactions are spontaneous (favorable)? a. 2H2O(g)⟶2H2(g)+O2(g) Δ𝐺=457 kJ/mol b. CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) Δ𝐺=−820 kJ/mol c. 2Mg(s)+O2(g)⟶2MgO(s) Δ𝐺=−1137 kJ/mol d. C(s)+H2O(l)⟶CO(g)+H2(g)

  3. Chemistry

    Use the information below to answer this question C(s) + O2(g) -> CO2(g) ΔH = -394 kJ/mol H2(g) + 1/2 O2(g) -> H2O(l) ΔH = -286 kJ/mol 4C(s) + 5H2(g) -> C4H10 (g) ΔH = -126 kJ/mol The standard enthalpy of combustion of butane,

  4. Chemistry - Science (Dr. Bob222)

    Hydrazine is used as a rocket fuel because its reaction with oxygen is extremely exothermic: N2H4(liquid) + O2(g)  N2(g) + 2H2O(liquid) ΔH(reaction) = -615 kJ mol-1 What is the enthalpy of this reaction if water were produced

  1. Chemistry

    According to the reaction 2Al+3H2SO4→3H2+Al2(SO4)3, the total number of moles of H2SO4 needed to react completely with 5.0 mol of AL is 1. 2.5 mol 2. 5.0 mol 3. 7.5 mol 4. 9.0 mol

  2. Chemistry

    Two reactions that occur in the production of iron (Fe) are 2 C + O2 → 2 CO followed by Fe2O3 + 3 CO → 2 Fe + 3 CO2 . Note that the carbon monoxide (CO) formed in the first reaction is then used in the second reaction.

  3. Chemistry

    A reaction between gaseous sulfur dioxide and oxygen gas to produce gaseous sulfur trioxide takes place at 600◦C. At that temperature, the concentration of SO2 is found to be 1.14 mol/L, the concentration of O2 is 1.39 mol/L,

  4. chemistry

    Fe2O3(s) + 3 CO(g) −→ 2 Fe(s) + 3 CO2(g) Given: 2 Fe2O3(s) −→ 4 Fe(s) + 3 O2(g) ∆H = 1616.6 kJ/mol CO(g) −→ C(s) + 1 2 O2(g) ∆H = 110.5 kJ/mol C(s) + O2(g) −→ CO2(g) ∆H = −393.5 kJ/mol Answer in units of

  1. AP CHEMISTRY

    Consider the reaction. PbCO3(s) PbO(s) + CO2(g). calculate the equilibrium pressure of CO2 in the system at the following temperatures.(IN atm) (a) 270°C (b) 480°C ..... delta Hf(KJ/mol).. d.Gf(KJ/mol).. S(J/mol-K)

  2. AP Chemistry

    For the reaction ? C6H6 + ? O2 ↽⇀? CO2 + ? H2O a maximum of ? moles of CO2 could be formed from 9 mol of C6H6 and 2.81 mol of O2. Answer in units of mol

  3. Chemistry

    An equilibrium mixture contains 0.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) + H2O(g) CO2(g)+ H2(g) How

  4. chemistry

    last check: (c) A wine cooler contains 4.5% ethanol by mass. Assuming that only the alcohol burns in oxygen, how many grams of wine cooler need to be burned to produce 3.12 L of CO2 (d = 1.80 g/L at 25°C, 1 atm pressure) at the

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