CH4 + 2O2 -> CO2 + 2H2O + heat If 5 mole of methane (CH4
Apr 25, 2018 · O_2 = 10 moles FIRST we make sure that the equation is balanced. Then we compare the coefficients of the compounds to find the molar ratios of reaction. CH_4 + 2O_2 -> CO_2 + 2H_2O is already balanced, so we only need to look at the ratio of methane and oxygen. CH_4 : O_2 = 1:2 or O_2 = 2xxCH_4 So, for 5 moles of …
#CH_4 +2O_2 ->CO_2 + 2H_2O# - Socratic
Mar 25, 2018 · Are there not "TWO moles" with respect to water? You have already written the stoichiometric equation that illustrates the combustion of methane gas... CH_4(g) + 2O_2(g) rarr CO_2(g) + 2H_2O(l) And this tells you UNEQUIVOCALLY, that 16*g of methane gas reacts with 64*g of dioxygen gas to give 44*g of carbon dioxide gas, and 36*g of water. As always in a chemical reaction, MASS and charge are ...
What mass of oxygen is required to react completely with 1.
Mar 7, 2018 · #CH_4(g) + 2O_2(g) rarr CO_2(g) +2H_2O(l) + Delta#...and given the stoichiometry if I completely combust a #1.2*mol# quantity of methane, then CLEARLY I get a molar quantity of #1.2*mol# with respect to carbon dioxide...and a #2.4*mol# quantity of water....
How many moles of hydrogen are there in 25.3 g of methane, …
Dec 17, 2017 · The answer is that there are 6.32 mol of hydrogen in 25.3 g of CH_4. First step is to find the molar mass of methane: Carbon is 12, hydrogen is 1, so CH_4 is 12+4xx1=16 Find the number of moles of CH_4 in 25.3 g: n=m/M=25.3/16=1.58 mole In each mole of CH_4 there are 4 moles of hydrogen, so our answer is 4xx1.58=6.32 mol
How do you calculate the partial pressures of this problem?
Aug 13, 2016 · A mixture containing 2.53 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C. (a) Calculate the partial pressure of each of the gases in the mixture. (b) Calculate the total pressure of the mixture. Answers in atmospheres.
A sample of gas contains 0.2000 mol of CH4 (g) and 0.4000 mol of …
Mar 8, 2018 · A sample of gas contains 0.2000 mol of CH4(g) and 0.4000 mol of O2(g) and occupies a volume of 20.3 L. The following reaction takes place: CH4(g) + 2O2(g)CO2(g) + 2H2O(g) Calculate the volume of the sample after the reaction takes place in liters?
Hydrogen gas (2.02 g/mol) can be produced from the reaction
Feb 25, 2018 · V = 1948.8L That is the "water shift" reaction. The balanced equation already given. With "excess" H_2O stipulated, we only need to convert the mass of the methane to the number of moles, then use the equation to find the number of moles of H_2 formed. With that value we use the ideal gas law to with the given temperature and pressure to find the actual volume of H_2 produced. 210g/16.05 = 13 ...
When 66.8g of (O2) gas is mixed with 27.8g of (NH3) gas and
Mar 27, 2018 · When 66.8g of (O2) gas is mixed with 27.8g of (NH3) gas and 25.1g of (CH4) gas, 36.4g of (HCN) gas is produced. What is the percent yield of HCN in this reaction? Chemistry
How many moles of carbon dioxide is formed when 4.0 moles of
May 23, 2017 · 4.0 mol "CO"_2 The chemical equation for this reaction is "H"_2"CO"_3"(aq)" rightleftharpoons "CO"_2"(g)" + "H"_2"O(l)" You'll notice that all the reagents in this reaction have equal amounts of relative moles, so if 4.0 moles of H_2CO_3 decomposes completely, there will be 4.0 moles of each water and carbon dioxide produced.
Why can some molecules have polar bonds, but overall be
Dec 7, 2015 · Symmetry. Look at methane for example. CH4. The bonds between carbon and the hydrogens are polar bonds, but the positioning of the hydrogens disperses any partial positive charge equally around the partially negative center, making the molecule non polar.