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
For the following reaction, if O2 is used up at a rate of 3.82Mhr, what is...
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 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 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...
How many moles of CH3OH are needed to react with 6 moles of O2 in the following equation? 2CH3OH + 3O2 -------> 2CO2 + 4H2O
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
Use Hess’s law to calculate ∆H° for the reaction:C(s) + 2H2(g) + ½O2(g) → CH3OH(l) ∆H°∘= ?using only the following data:H2(g) + ½O2(g) → H2O(l) ∆H°= -285.8 kJC(s) + O2(g) → CO2(g) ∆H°= -393.5 kJ2CH3OH(g) + 3O2(g) → 2CO2(g) + 4H2O(l) ∆H°= -1452.8 kJ
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
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%
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.