What is the enthalpy of the reaction for the following equation:
2CH3OH(l) + 3O2(g) -----> 2CO2(g) + 4H2O(g)
Given the following bond enthalpies (in kj/mol): C-H (414); C-O (360); C=O (799); O=O (498); O-H (464). Note: O=C=O
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What is the enthalpy of the reaction for the following equation: 2CH3OH(l) + 3O2(g) -----> 2CO2(g)...
Consider the balanced equation for the following reaction: 3O2(g) + 2CH3OH(l) → 2CO2(g) + 4H2O(l) If O2 is present in excess, determine the amount of CH3OH needed to produce 3.22 moles of H2O. A) 0.403 moles B) 1.49 moles C) 6.44 moles D) 2.18 moles E) 1.61 moles
For the following reaction: 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH3OH (l) -238.40 127.19 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 H2O (l) -285.83 69.91 Determine the temperature (to two decimal places in K) such that the reaction is in equilibrium in its standard states.
Consider the following balanced equation: 3O2(g) + 2CH3OH(l) → 2CO2(g) + 4H2O(l) If 30.3 moles of O2(g) and 31.1 moles of CH3OH(l) are allowed to react to produce 15.0 moles of CO2(g), what is the percent yield of the reaction? a-57.5% b-74.3% c-48.1% d-85.0% e-70.2%
Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l), ΔH°rxn = –1454 kJ/mol. A) How much heat, in kilojoules, is given off when 150.0 g of methanol is burned? [ Select ] B) How many grams of CO2 are produced when the amount of heat determined in part A is released? [ Select ] Molar masses: CH3OH = 32.04 g/mol O2 = 32.00 g/mol CO2 = 44.01 g/mol H2O = 18.02 g/mol
Methanol is combusted to provide heat. The reaction and the enthalpy for the reaction are shown below. CH3OH(l)+1.5O2(g)→CO2(g)+2H2O(l)ΔH=−715kJ Below is a list of sentences that describe a chemical reaction. Choose all of the sentences that apply to the above reaction. Check all that apply. View Available Hint(s) Check all that apply. The enthalpy for 2CH3OH(g)+3O2(g)→2CO2(g)+4H2O(l) is −715 kJ The enthalpy for 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(l) is 715 kJ This process is endothermic. The enthalpy for 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(l) is −1,430 kJ This chemical reaction transfers...
3O2(g) + 2CH3OH(l) → 2CO2(g) + 4H2O(l) Determine the amount of CO2(g) formed in the reaction if 4.20 moles of O2(g) reacts with an excess of CH3OH(l) and the percent yield of CO2(g) is 70.0%. A. 1.86 moles B. 3.57 moles C. 4.00 moles D. 1.96 moles E. 2.16 moles
Given the following reaction: CH3CH2OH(l)+3O2(g)→2CO2(g)+3H2O(l)CH3CH2OH(l)+3O2(g)→2CO2(g)+3H2O(l) ∆H = –2200 kJ/mol CH3CH2OHCH3CH2OH a) This reaction is... Select one or more: a. exothermic b. endothermic
predict the enthalpy of reaction from the average bond enthalpies for the following reaction 2C2H6(g) + 7O2(g) ---> 4CO2(g) + 6H2O(g) ( in kJ) Bond Enthalpy (kJ/mol) H-H 436.4 H-O 460 C-H 414 C-C 347 C=C 620 C-O 351 O-O 142 O=O 498.7 C=O 745 C=O 799 (carbon dioxide)
At 298 K, evaluate deltaG(kJ) and deltaE (V) for 2CH3OH(l) + 3O2(g) -> 4H2O(g) + 2CO2(g) S (J/mol-K) AH°y (kJ/mol) So (J/mol-K) AH(kJ/mol) Substance Substance N2(g) CH-ОН() 126.8 0 191.5 -238.6 CO(g) NH3(g) 197.9 192.5 -110.5 -46.2 CO2(g) NO(g) 213.6 +90.4 210.6 -393.5 NO2(g) +33.8 240.5 H2(g) HNO3(aq) 130.6 146.0 -206.6 H2O( 69.9 -285.8 O2(g) 188.8 H2O(g) 0 205.0 -241.8
Methanol (CH3OH) burns in air according to the equation 2CH3OH + 3O2 → 2CO2 + 4H2O If 167 g of methanol are used up in a combustion process, what is the mass of H2O produced