Consider the chemical reaction: C(s)+H2O(g)→CO(g)+H2(g) How many liters of hydrogen gas are formed from the complete...

Consider the chemical reaction: C(s)+H2O(g)→CO(g)+H2(g)

How many liters of hydrogen gas are formed from the complete reaction of 1.16 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and temperature of 319 K. ( ANSWER SHOULD BE IN LITERS )

Express your answer using two significant figures.

CH3OH can be synthesized by the reaction:
CO(g)+2H2(g)→CH3OH(g)

How many liters of H2 gas, measured at 741 mmHg and 88 ∘C, are required to synthesize 0.68 mol of CH3OH?

Express your answer using two significant figures.

How many liters of CO gas, measured under the same conditions, are required?

How many grams of NH3 form when 24.5 L of H2(g) (measured at STP) reacts with N2 to form NH3 according to this reaction?
N2(g)+3H2(g)→2NH3(g)

The mass of an evacuated 255 mL flask is 143.227 g . The mass of the flask filled with 263 torr of an unknown gas at 35 ∘C is 144.247 g .

Calculate the molar mass of the unknown gas.

Solutions

Expert Solution

1) C(s) +H2O(g) ----- CO(g) + H2(g)
1 mole 1 mole
according to equation
1 mole of C= 1 mole of H2
1.16 mole of C = ?
=1.16x1/1=1.16 mole
number of moles of H2= 1.16 moles
Pressure =P= 1.0atm
Temperature = T= 319 K
gas constant = R= 0.0821 L-atm/mol-K
PV=nRT
V= nRT/P = 1.16x0.0821x319/1.0 = 30.38L
Volum of Hydrogen gas = 30.38L=30L

2) CO(g) + 2H2(g) -------- CH3OH(g)
2 mole 1 mole
according to equation
1 mole of CH3OH = 2 mole of H2
0.68 mole of CH3OH =?
= 2x0.68/1=1.36 mole
number of moles of H2= 1.36 moles
Pressure =P= 741mm=741/760=0.975 atm
T=88C=88+273=361K
R=0.0821 L-atm/mol-K
Pv=nRT
V=nRT/P
V= 1.36 x0.0821x361/0.975=41.34L
Volume of H2= 41L

according to equation
1 mole of CH3OH= 1mole of CO
0.68 mole of CH3OH= 0.68 mole of CO
n=0.68 mole
V= 0.68x0.0821x361/0.975= 20.67L
Volume of CO = 20.67L = 21L

queen_honey_blossom answered 1 year ago

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