Consider the chemical reaction: C( s )+H2O( g )CO( g )+H2( g ) Part A How many l

Question

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

Part A

How many liters of hydrogen gas are formed from the complete reaction of 1.09 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and temperature of 313 K .

Express your answer using two significant figures.

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

Part A

How many liters of hydrogen gas are formed from the complete reaction of 1.09 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and temperature of 313 K .

Express your answer using two significant figures.

Explanation / Answer

C(s)+H2O(g)CO(g)+H2(g)

according to balanced reaction

1 mole C gives 1 mole H2

1.09 moles C gives 1.09 moles H2

convert moles to L

PV = nRT

V = nRT/P

V = (1.09 x 0.0821 x 313 / 1.0)

V = 28.0 L

VH2 = 28.0 L

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects