Are the following two balanced?
-2 NaHCO3 ? Na2 CO3 + H2O + 2 CO2
-CH4 + 2 O2 = CO2 + 2 H2O
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Are the following two balanced? -2 NaHCO3 ? Na2 CO3 + H2O + 2 CO2 -CH4...
The reaction of NaHCO3 and HCl produces NaCl, H2O and CO2. The balanced equation is: NaHCO3 + HCl = NaCl + H2O + CO2 You combine 5.0 g of NaHCO3 and 5.0 g of HCl. Determine the limiting reagent. Determine the amount of NaCl formed in the reaction based on these quantities of reactants. How much of the excess reactant remains? Thank you in advance!
From the following balanced equation, H₂ = 1.0144 CH4 () +202) - CO2(g) + 2 H2O(8) How many grams of H20 can be formed when 1.25 g CH are combined with 6.66 g0,?
Which of the following processes have a ΔS > 0? A) Na2CO3(s) + H2O(g) + CO2(g) → 2 NaHCO3(s) B)CH4(g) + H2O(g) → CO(g) + 3 H2(g) C)CH3OH(l) → CH3OH(s) D)N2(g) + 3 H2(g) → 2 NH3(g) E)All of the above processes have a DS > 0.
Consider the following reaction: CH4 + 2 O2 → CO2 + 2 H2O b) Determine the number of moles of oxygen that would be needed to react with the methane in part A. ( Calculate the number of moles in 28.4 g of methane. )
Which of the following species acts as a reducing agent during the following reaction? CH4(g)+O2(g)⟶CO2(g)+H2O(l) Options: (a) CH4 (b) O2 (c) CO2 (d) H2O
Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) CO2(g) 214 H2O(l) 189 CH4(g) 186 O2(g) 205
Which of the following equations correctly describes the combustion of methane (CH4) gas? a. CH4 + 1/2O2 --> CO2 + H2O b. CH4 + O2 --> CO2 + H2O C. CH4 + O2 --> CO2 + 2 H2O d. CH4 + 2 O2 --> CO2 + 2 H2O e. CH4 + 3 O2 --> 2 CO2 + H2O
When NaHCO3 is heated above 270 °C, it decomposes to Na2CO3, H2O, and CO2. Write a balanced chemical equation for the decomposition reaction. Do not include phases.Calculate the mass of CO2 produced from the decomposition of 21.00 g of NaHCO3.
CH4 (g) + O2(g) +H2O-------> CO2 (g) + H2O What would the percent yield of the reaction be if 15.2 g of O2 were reacted and only 6.7 g of CO2 were made?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) Calculate ΔH for the reaction using the bond enthalpies given. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) Calculate the overall enthalpy change for this reaction using the bond enthalpies given.