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%
Consider the following balanced equation: 3O2(g) + 2CH3OH(l) → 2CO2(g) + 4H2O(l) If 30.3 moles of...
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
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
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
Consider the reaction for the combustion of methanol (CH3OH): 2CH3OH+3O2⟶2CO2+4H2O What is the mass of oxygen (O2) that is required to produce 579g of carbon dioxide (CO2)?
1. Consider the balanced equation for the following reaction: 302(g) + 2CH3OH() → 2CO2(g) + 4H2O(1) If 3.77 moles of O2 reacts with 2.66 moles of CH3OH, determine how much excess reactant remains in the reaction 1.33 moles 2.00 moles 0.15 moles 1.40 moles 2.66 moles Use the slider to rate your confidence on this question. 100 Not at all confident Very confident
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.
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
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
Consider the following balanced chemical equation: C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) a. How many moles of CO2 form when 1.53 moles of C2H5OH react? moles CO2 b. How many moles of H2O form from the reaction of 1.53 moles of C2H5OH? moles H2O c. How many moles of CO2 form when 1.53 moles of H2O form? moles CO2 d. How many molecules of CO2 form when 1.53 moles of H2O form? × 10(Click to select)21222324 molecules CO2
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