Question

In: Chemistry

Methanol (CH3OH) is made industrially in two steps from CO and H2. It is so cheap...

Methanol (CH3OH) is made industrially in two steps from CO and H2. It is so cheap to make that it is being considered for use as a precursor to hydrocarbon fuels such as methane (CH4): Step 1. CO(g)+2H2(g)→CH3OH(l) ΔS∘ = -332J/K Step 2. CH3OH(l)→CH4(g)+1/2O2(g) ΔS∘ = 162J/K

a. Calculate an overall ΔG∘ for the formation of CH4 from CO and H2.

b. Calculate an overall ΔH∘ for the formation of CH4 from CO and H2.

c. Calculate an overall ΔS∘ for the formation of CH4 from CO and H2

d. is the overall reaction spontaneous?

e. If you were designing a production facility, would you plan on carrying out the reactions in separate steps or together?

f.

Solutions

Expert Solution

Comment in case of any doubt.


Related Solutions

Methanol (CH3OH) is made industrially in two steps from CO and H2. It is so cheap...
Methanol (CH3OH) is made industrially in two steps from CO and H2. It is so cheap to make that it is being considered for use as a precursor to hydrocarbon fuels such as methane (CH4): Step 1. CO(g)+2H2(g)→CH3OH(l) ΔS∘ = -332J/K Step 2. CH3OH(l)→CH4(g)+1/2O2(g) ΔS∘ = 162J/K a) Calculate an overall ΔG∘ for the formation of CH4 from CO and H2H2. b) Calculate an overall ΔH∘ for the formation of CH4 from CO and H2. c) Calculate an overall ΔS∘...
Methanol is prepared industrially from synthesis gas (CO and H2). CO(g) + 2H2(g) ⇌ CH3OH(g); ΔH°...
Methanol is prepared industrially from synthesis gas (CO and H2). CO(g) + 2H2(g) ⇌ CH3OH(g); ΔH° = -21.7 kcal Would the fraction of methanol obtained at equilibrium be increased by raising the temperature? Explain.
Methanol (CH3OH) is made by reacting gaseous carbon monoxide (CO) and gaseous hydrogen (H2). A. What...
Methanol (CH3OH) is made by reacting gaseous carbon monoxide (CO) and gaseous hydrogen (H2). A. What is the theoretical yield of methanol if you react 37.5 kg of CO(g) with 4.60 kg of H2(g)? B. You found that 1.83 x 104 g of methanol is actually produced. What is the percent yield of methanol?
Methanol, CH3OH, can be made from the reaction of carbon monoxide and hydrogen. CO(g) + 2...
Methanol, CH3OH, can be made from the reaction of carbon monoxide and hydrogen. CO(g) + 2 H2(g) → CH3OH(l) What mass of hydrogen is required to produce 3.50 L of methanol (d = 0.791 g/mL) if this reaction has a 73.01% yield under certain conditions?
Methanol (CH3OH) is produced by reacting carbon monoxide (CO) and hydrogen (H2). A fresh feed stream...
Methanol (CH3OH) is produced by reacting carbon monoxide (CO) and hydrogen (H2). A fresh feed stream containing CO and H2 joins a recycle stream and the combined stream is fed into a reactor. The reactor outlet stream flows at a rate of 350 mol/min and contains 10.6 wt% H2, 64.0 wt% CO, and 25.4 wt% CH3OH. The stream enters a cooler in which most of the methanol is condense. The liquid methanol is withdrawn as a product, and the gas...
CH3OH can be synthesized by the following reaction. CO(g)+2H2(g)→CH3OH(g) What volume of H2 gas (in L),...
CH3OH can be synthesized by the following reaction. CO(g)+2H2(g)→CH3OH(g) What volume of H2 gas (in L), measured at 746 mmHg and 84 ∘C, is required to synthesize 23.4 g CH3OH? How many liters of CO gas, measured under the same conditions, is required?
XP10. Methanol (CH3OH) can be used as an antifreeze or fuel and can be synthesized from...
XP10. Methanol (CH3OH) can be used as an antifreeze or fuel and can be synthesized from carbon monoxide (CO) and hydrogen (H2). The product from a reactor contains CO, H2, CH2OH, and 102 mol/h N2 (an inert component). The total flow rate of the feed to the reactor is 476 mol/h, and the feed contains an equal molar flow rate of CO and H2. The total flow rate exiting the reactor is 318 mol/h. (a) Draw and label a process...
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) The reaction between CO and H2 is carried out at a...
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) The reaction between CO and H2 is carried out at a specific temperature with initial concentrations of CO = 0.32 M and H2 = 0.53 M. At equilibrium, the concentration of CH3OH is 0.16 M. Part A Find the equilibrium constant at this temperature. Express your answer using two significant figures.
The two most commonly used antifreezes are methanol (CH3OH), and ethylene glycol (CH2OH)2. Calculate the mass...
The two most commonly used antifreezes are methanol (CH3OH), and ethylene glycol (CH2OH)2. Calculate the mass of each solute required to depress the freezing point of exactly 1000 grams of water by 12 °F. Please give a detailed explanation.
10. How much methanol (CH3OH, in grams) can be formed from 49.2 mg of hydrogen? Assume...
10. How much methanol (CH3OH, in grams) can be formed from 49.2 mg of hydrogen? Assume excess CO. CO(g) + 2H2(g) → CH3OH(g) -Consider the following balanced chemical equation: 2N2H4(g) + N2O4(g) → 3N2(g) + 4H2O(g) a. How many moles of water form from 0.438 moles of N2O4? b. How many moles of water form from 0.438 moles of N2H4? c. How many moles of nitrogen form from 0.438 moles of N2O4? d. How many moles of nitrogen form from...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT