How many moles of CH3OH are needed to react with 6 moles of O2 in the following equation?
2CH3OH + 3O2 -------> 2CO2 + 4H2O
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In the reaction below how many moles of water would be produced
if you used 3 moles of oxygen gas (O2) and much CH3OH as needed to
react with all the oxygen 2CH3OH + 3O2
2CO2 + 4H2O
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 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, if O2 is used up at a rate of 3.82Mhr, what is the rate of consumption of CH3OH? 2CH3OH+3O2→2CO2+4H2O
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
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)?
What mass of water (in units of grams) is produced by the reaction of 5.25g CH3OH with an excess of O2 when the percent yield is 41.4%? 2CH3OH (g) + 3O2 (g) -> 2CO2 (g) + 4H2O (l)
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 (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
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