Download the App!

Get 24/7 study help with the Numerade app for iOS and Android! Enter your email for an invite.

Industrially, hydrogen gas can be prepared by reacting propane gas $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ with steam at about $400^{\circ} \mathrm{C} .$ The products are carbon monoxide (CO) and hydrogen gas ( $\mathrm{H}_{2}$ ). (a) Write a balanced equation for the reaction. (b) How many kilograms of $\mathrm{H}_{2}$ can be obtained from $2.84 \times 10^{3} \mathrm{kg}$ of propane?

Get the answer to your homework problem.

Try Numerade free for 7 days

Like

Report

a) $\mathrm{C}_{3} \mathrm{H}_{8}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow 3 \mathrm{CO}+7 \mathrm{H}_{2}$b) $915.3 \mathrm{kg}$

Chemistry 101

Chapter 3

Mass Relationships in Chemical Reactions

Chemical reactions and Stoichiometry

University of Maryland - University College

University of Kentucky

University of Toronto

Lectures

04:02

A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Chemical reactions can be either spontaneous, requiring no input of energy, or non-spontaneous, typically following the input of some type of energy, such as heat, light or electricity. Chemical reactions are usually characterized by a chemical change, and they yield one or more products after the reaction is complete. Chemical reactions are described with chemical equations, which symbolically present the starting materials, end products, and sometimes intermediate products and reaction conditions. Chemical reactions happen at a characteristic reaction rate at a given temperature and chemical concentration. Typically, reaction rates increase with increasing temperature because there is more thermal energy available to reach the activation energy necessary for breaking bonds between atoms.

08:02

In chemistry, a combination reaction is a chemical reaction in which two or more reactants combine to form more than one product. In a decomposition reaction, one reactant splits into two or more products.

03:56

Industrially, hydrogen gas…

04:39

Propane gas, $\mathrm{C}_{…

01:39

04:38

03:59

Propane $\left(\mathrm{C}_…

Given information for part, a c 3 h, 8 plus h, 2, o carbon monoxide plus h 2, so we have to write the balance equation for a given reaction. So here we have to balance the given reaction. We have 3 carbon atoms on the reactant side and 1 carbon atom on the product side, so we will place 33 in front of c and g. We will put 3 in front of c o and get here the equation: c: 3 h, 8, plus h, 2. O and you put 3 in front of co plus h 2 point now: we have 3 oxygen, 3 oxygen, 3 oxygen product side and 1 reactant side, so we will place 3 in front of h. 2, o ye place 3 in front of h, 2 o. So the reaction become c: 3, h, 8 plus 3 h, 2, o into 32 co, plus h, 2 point. Finally, we have 14 hydrogen 14 hydrogen atom and reacting side 8 here in 6 year year, total 14 hydrogen atoms and reactant side and 2 product side. So we will place 1 in front of h 2 and get the balance equation here. The balance equation c: 3, h, 8 plus 3, h, 2, o into 3 co, plus 7. H, 2 point. So the balance ecclesian here the number of carbon atoms are balanced. Number of hydrogen atoms are balanced and number of oxygen. Atoms are also balanced here and given information for part b. The mass of propane is mass of propane c. 3. H 8 is equal to 2.84 into 10 raised to the power. 31 kg is equal to 2.86 into 10, raise to the power 6 g convert kg into gram. Here and now we have to calculate the mass of h, 2 produces by a given amount of propine. So first we will find the numbers of moles are propanso. The molar mass molar mass of propane isamassopropane is equal to 3 into molar mass of carbon plus 8 into molar. Mass of hydrogen is equal to 3 into molar. Mass of carbon is 12 into 011 gram per mole plus 8 into 1.008. Gram per mole is the molar mass of hydrogen is equal to m f. We have 44 in the calculated molar. Mass of propine is 44.097 gram per mole, and the number of moles of propane is number of moles of prois equal to a divided by molar. Mass of propane is equal to 2.86. A .10 raised to the power 6 gram divided by 44.097 gram per mole, is equal to is equal to 6.486 into 10 raised to the power 4 molesince 1 molapropaine produces 7 molah 2. Since 1, mole of propane produces 7 moles of h 26.486 into 10, raised to the power 4 moles of propane will produce will produce. We have here. Number of moles of hydrogen is equal to 7. Point number of moles of is equal to 7 into 6486 into 10. Raise to the power 4 is equal to 45.40 into 10, raise to the power 4 moltherefore. The mass of h 2 is they are for number. The number of, therefore, the mass of h. 2 h 2 is the mass of h. 2 is equal to the number of moles of h 2 into molar. Mass of h. 2 is equal to moles of number of moles. Of h. 2 is 45.402 mole into 10 raised to the power 4 into 2.016. Gram per mole is equal to 91.53 into 10 raised to the power 4 gram is the calculated mass of h. 2 is equal to 915.3, the calculated mass of s 2. So we have the final result for part. A is c 3 h, 8 plus 3 h, 2, o and 3 co, plus 7 h, 2 and final result for part b is 915.3 kilogram? Is the mass of.

View More Answers From This Book

Find Another Textbook

Numerade Educator