   Chapter 13, Problem 90QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
1 views

# Calcium carbide, CaC 2 , reacts with water to produce acetylene gas, C 2 H 2 .msp;  CaC 2 ( s ) + 2H 2 O ( l )   C 2 H 2 ( g ) + Ca ( OH ) 2 ( s ) at volume of acetylene at 25  ° C and 1 .0 1 atm is generated by the complete reaction of 2 . 49 g of calcium carbide? What volume would this quantity of acetylene occupy at STP?

Interpretation Introduction

Interpretation:

The volume of acetylene at given temperature and at STP should be calculated.

Concept Introduction:

According to ideal gas equation:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

The value of Universal gas constant can be taken as 0.082 L atm K1 mol1.

Mass of gas can be calculated from number of moles and molar mass as follows:

m=n×M

Here, n is number of moles, m is mass and M is molar mass.

Explanation

Calculation:

The balanced chemical reaction is as follows:

CaC2(s)+2H2O(l)C2H2(g)+Ca(OH)2(s)

To calculate the volume of acetylene, first calculate the number of moles of calcium carbide as follows:

n=mM

Molar mass of calcium carbide is 64.099 g/mol.

Putting the value,

n=2.49 g64.099 g/mol=0.0388 mol

From the balanced chemical reaction, 1 mol of calcium carbide gives 1 mol of acetylene thus, number of moles of acetylene produced from 0.0388 mol of calcium carbide will be 0.0388 mol.

Volume can be calculated from ideal gas equation as follows:

V=nRTP

Convert the given temperature from C to K as follows:

0 C=273.15 K

Thus,

25 C=(25+273

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