Consider the gas phrase reaction shown below:
CH4(g) + 2O2 (g) -> CO2(g) + 2H2O (g)
Write the rate expression in terms of the rate of appearance of CO2
Rate= ? M/s
If the average rate of disapperace of O2 is Δ[O2]/ Δt = -.0400 M/s, calculate the average rate of appearance of CO2 over the same time interval
Δ[CO2]/ Δt= ? M/s
(Please show all work! thank you!)
Consider the gas phrase reaction shown below: CH4(g) + 2O2 (g) -> CO2(g) + 2H2O (g)...
In the reaction CO2(g) + 2H2O(g) ? CH4(g) + 2O2(g) the initial rate of change in the concentration of CO2 is ?3.2 × 10?5 M s?1. What are the initial rates of change in the concentration of the other three substances in the reaction mixture?
Use the example shown to calculate the reaction enthalpy, delta H, for the following reaction: CH4(g)+2O2(g)->CO2(g)2H2O(l). Use the series of reaction that follows: 1. C(s)+2H2(g)-> CH4(g), delta H= -74.8 kJ 2. C(s)+O2(g)->CO2(g), delta H= -393.5 kJ 3. 2H2(g)+O2(g)-> 2H2O(g), delta H= -484.0 kJ 4. H2O(l)->H2O(g), delta H= 44.0 kJ
Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product ΔH∘f (kJ/mol) CH4(g) -201 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units.
please help Consider following chemical reactions: 1) CH.(g) + 2O2(g) → CO2(g) + 2H2O(1) 2) C(s) + O2(g) → CO2(g) 3) 2C(s) + O2(g) - 200(g) 4) 3C(s) + 2H2O) CH4(g) + 2COg) H2O(l) indicates that H20 is in liquid state. If the Enthalpy of reaction for reaction 1, 2, and 3 are -890.4kj, -393.5kj and - 221.Okj respectively; try to figure out the Enthalpy of reaction for reaction 4. Please show your work.
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g).
Calculate ΔrH for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(l) Use the following reactions and given ΔrH's. CH4(g)+O2(g)→CH2O(g)+H2O(g), ΔrH = -284 kJmol−1 CH2O(g)+O2(g)→CO2(g)+H2O(g), ΔrH = -527 kJmol−1 H2O(l)→H2O(g), ΔrH = 44.0 kJmol−1
For the reaction CH4 + 2O2 → CO2 + 2H2O, how many moles of carbon dioxide are produced from the combustion of 97.0 g of methane?
CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H = -882 kJ/mol From the equation above, What is Δ H for the reaction below in kJ/mol. H2O (g)+ 1/2 CO2 (g) --> O2 (g) + 1/2 CH4 (g)
What mass of natural gas (CH4) must you burn to emit 258 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g): 572 kJ -801 kJ -572 kJ 801 kJ