   Chapter 13, Problem 156CP ### 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
18 views

# onsider the unbalanced chemical equation:msp;  CaSi 3 ( s ) + HF ( g )   CaF 2 ( a q ) + SiF 4 ( g ) + H 2 O ( l ) ppose a 32 . 9 − g sample of CaSiO 3 is reacted with 31 . 8 L of HF at 27 .0   ° C and 1 .00 atm. Assuming the reaction goes to completion, calculate the mass of SiF4and H 3 O produced in the reaction.

Interpretation Introduction

Interpretation:

To calculate mass of SiF4 and H2O formed during the reaction.

Concept Introduction:

Mole concept represents the mole ratio of products and reactants with the help of molar mass. The relation between mass and moles can be written as;

number of moles= massmolar mass.

Explanation

Given information:

Mass of CaSiO3 = 32.9 g

Volume of HF = 31.8 L

Temperature = 27 Â°C = 273+27 = 300 K

Pressure = 1 atm

We need to calculate the moles of each reactant and determine the reactant that limits the reaction. Here CaSiO3 is limiting reagent therefore it will determine the amount of product formed.

Moles of CaSiO3 = mass gmolar mass = 32.9 g172.24 g/mol = 0.19 moles

Moles of HF = Pressure×Volumegas constant×temperature

Moles of HF = 1 atm×31.8 L0.0821 atm/K.mol×300 K

Moles of HF = 1.29 moles

Since, moles of CaSiO3 is less hence it will limit the reaction and determine the amount of product

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 