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

Question

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

Part A

How many liters of hydrogen gas is formed from the complete reaction of 18.8 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K .

Express your answer using two significant figures.

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

Part A

How many liters of hydrogen gas is formed from the complete reaction of 18.8 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K .

Express your answer using two significant figures.

Explanation / Answer

A)

Molar mass of C = 12.01 g/mol

mass of C = 18.8 g

mol of C = (mass)/(molar mass)

= 18.8/12.01

= 1.5654 mol

From balanced chemical reaction, we see that

when 1 mol of C reacts, 1 mol of H2 is formed

mol of H2 formed = moles of C

= 1.5654 mol

we have:

P = 1.0 atm

n = 1.5654 mol

T = 360.0 K

we have below equation to be used:

P * V = n*R*T

1 atm * V = 1.5654 mol* 0.08206 atm.L/mol.K * 360 K

V = 46 L

Answer: 46 L

Feel free to comment below if you have any doubts or if this answer do not work. I will edit it if you let me know

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