Question

The reaction of coal and water at a high temperature produces a mixture of hydrogen and...

The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as Synthesis gas (or syngas). What mass of carbon monoxide can be formed from the reaction of 71.3 g of carbon with excess water?
C(s) +H2O H2(g) + CO(g)

Homework Answers

Answer #1

Solution :-

Balanced reaction equation

C(s) + H2O(l) --- > H2(g) + CO(g)

Using the given mass of carbon we can find the mass of                carbon monoxide that can be formed by using the stoichiometric mole ratio of the C and CO.

Lets set up the equation and calculate the mass of CO that can be formed using the 71.3 g Carbon

(71.3 g C * 1 mol / 12.01 g)*(1 mol CO / 1 mol C)*(28.01 g / 1 mol CO) = 166 g CO

Therefore the mass of the carbon monoxide (CO) that can be formed is 166 g CO

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Making Hydrogen Gas ​Passing steam over hot carbon produces a mixture of carbon monoxide and hydrogen:...
Making Hydrogen Gas ​Passing steam over hot carbon produces a mixture of carbon monoxide and hydrogen: H2O(g) + C(s) <=> CO(g) + H2(g) The value of Kc for the reaction at 1000°C is 3.0 × 10–2. a. Calculate the equilibrium partial pressures of the products and reactants if PH2O = 0.442 atm    and PCO = 5.0 atm at the start of the reaction. Assume that the carbon is in excess. b. Determine the equilibrium partial pressures of the reactants...
3. The water-gas reaction is used to produce combustible gases from carbon (coal) and steam. C(s)...
3. The water-gas reaction is used to produce combustible gases from carbon (coal) and steam. C(s) + H2O(g) CO(g) + H2(g) Kp = 9.7x10-17 at 298 K Ho = 131 kJ What will the effect on the final equilibrium amount of H2(g) if a gaseous mixture originally at equilibrium with a large excess of C(s) at 298 K is subjected to the following changes: (increase, decrease or no change) How can I tell can I have an reason why it...
SHOW COMPLETE AND CLEAR SOLUTION thanks. The reaction: CO(g) + H2O(g) ⇔ CO2(g) + H2(g) is...
SHOW COMPLETE AND CLEAR SOLUTION thanks. The reaction: CO(g) + H2O(g) ⇔ CO2(g) + H2(g) is used to increase the ratio of hydrogen in synthesis gas (mixtures of CO and H2. Suppose you start with 1.00 mol each of carbon monoxide and water in a 50.0 L vessel. What is the concentration of each substance in the equilibrium mixture at 1000°C given that Kc = 0.58 at this temperature?
An equilibrium mixture contains 0.450 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.450 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container CO(g) + H2O(g) <===> CO2(g) + H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
An equilibrium mixture contains 0.650 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.650 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) + H2O(g) <-----> CO2(g) + H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
Large quantities of hydrogen are needed for the synthesis of ammonia. One preparation of hydrogen involves...
Large quantities of hydrogen are needed for the synthesis of ammonia. One preparation of hydrogen involves the reaction between carbon monoxide and steam at 3.00 × 102 °C in the presence of a copper-zinc catalyst: CO(g) + H2O(g) ⇆ CO2(g) + H2(g) Using the standard formation constant data in the table, calculate the equilibrium constant (KP) for the reaction at 3.00 × 102 °C and the temperature at which the reaction favors the formation of CO and H2O Species Δ...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.5 L of methane gas (measured at a pressure of 736 torr and a temperature of 25 ∘C) is mixed with 22.6 L of water vapor (measured at a pressure of 700 torr and a temperature of 125 ∘C). The reaction produces 26.0 L of hydrogen gas measured at STP. What is the percent...
How many liters of hydrogen gas are formed from 15.7g of carbon? Assume the hydrogen gas...
How many liters of hydrogen gas are formed from 15.7g of carbon? Assume the hydrogen gas is collected at a pressure 1.0atm and a temperature of 355K. C(s) + H2O (g) → CO(g) + H2 (g)
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.5 L of methane gas (measured at a pressure of 730 torr and a temperature of 25 ∘C) is mixed with 22.6 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 ∘C). The reaction produces 26.2 L of hydrogen gas measured at STP. What is the percent...
A) The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following...
A) The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following chemical equation: CO(g)+2H2(g)⇌CH3OH(g) The equilibrium constant for this reaction at 25 ∘Cis Kc=2.3×104. In this trial, you will use the equilibrium-constant expression to find the concentration of methanol at equilibrium, given the concentration of the reactants. Suppose that the molar concentrations for CO and H2 at equilibrium are [CO] = 0.04 M and [H2] = 0.04 M. Use the formula you found in Part...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT