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Chapter 3: Q3.133CP (page 137)

Hydrogen gas has been suggested as a clean fuel because it produces only water vapour when it burns.Ifthe reaction has a 98.8% yield, what mass of hydrogen forms 105 kg of water?

Short Answer

Expert verified

TheMass of hydrogen formed from of water is $1.19 脳 10^{4} g$

Step by step solution

01

Calculation of theoretical yield of the water vapors:

Given:

Percentage yield of water vapor = $98.8 %$

Mass of water = $105kg$

$Percentage yield= \frac{Actual yield of water}{Theoretical yield of water} 脳 100 Theoretical yield of water = \frac{Actual yield of water}{Percentage yield of water} 脳 100 Theoretical yield of water= \frac{105 kg}{98.8 %} 脳100 = 106 kg$

02

Step 2:Calculation of Hydrogen gas produced.

Let us calculate the mass of hydrogen gas from a theoretical yield of water.

$2 H_{2} ({g) +O}_{2} 鈫� 2 H_{2} O(g)$

Molar mass of $H_{2} O = 18.02 g/mol$

Molar mass of $H_{2} = 2.02 g/mol$

${1 kg = 10}^{3} g$

$106 kg = 106 脳 10^{3} g$

${Mass ofH}_{2} = 106 脳 10^{3} g 脳 \frac{1 {mol ofH}_{2} O}{18.02 {g ofH}_{2} O} 脳 \frac{2 {mol ofH}_{2}}{2 {mol ofH}_{2} O} 脳 \frac{2.02 {g ofH}_{2}}{{1mol ofH}_{2}}$

${Mass ofH}_{2} {=1.19脳10}^{4} g$

Result:

The mass of hydrogen gas produced is ${1.19脳10}^{4} g$

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Most popular questions from this chapter

Ethanol (CH₃CH₂OH), the intoxicant in alcoholic beverages, is also used to make other organic compounds. In concentrated sulfuric acid, ethanol forms diethyl ether and water:

$2 C H_{3} C H_{2} O H (I) 鈫� C H_{3} C H_{2} O C H_{3} C H_{2} (I) + H_{2} O (g)$

In a side reaction, some ethanol forms ethylene and water:

$C H_{3} C H_{2} O H (I) 鈫� C H_{2} = C H_{2} (g) + H_{2} O (g)$

(a) If 50.0 g of ethanol yields 35.9 g of diethyl ether, what is the percent yield of diethyl ether? (b) During the process, 45.0% of the ethanol that did not produce diethyl ether reacts by the side reaction. What mass of ethylene is produced?

3.14 Calculate each of the following quantities:
(a) Mass in grams of $6.44 脳 10^{- 2}$ mol of ${MnSO}_{4}$
(b) Moles of compounds in 15.8 kg of $Fe {({ClO}_{4})}_{3}$
(c) Number of N atoms in 92.6 mg of ${NH}_{4} {NO}_{2}$

Nitrogen monoxide reacts with elemental oxygen to form nitrogen dioxide. The scene at right represents an initial mixture of reactants. If the reaction has a 66% yield, which of the scenes below (A, B, or C) best represents the final product mixture?

When 20.5 g of methane and 45.0 g of chlorine gas undergo a reaction that has a 75.0% yield, what mass of chloromethane $({CH}_{3} Cl)$ forms? Hydrogen chloride also forms.

Aspirin (acetylsalicylic acid, C₉H₈O₄) is made by reacting salicylic acid (C₇H₆O₃) with acetic anhydride [(CH₃CO)₂O]:

$C_{7} H_{6} O_{3} (S) + {(C H_{3} C O)}_{2} O (I) 鈫� C_{9} H_{8} O_{4} (S) + C H_{3} C O O H (I)$

In one reaction, 3.077 g of salicylic acid and 5.50 mL of acetic anhydride react to form 3.281 g of aspirin. (a) Which is the limiting reactant (d of acetic anhydride = 1.080 g/mL)? (b) What is the percent yield of this reaction? (c) What is the percent atom economy of this reaction?

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