Given the following unbalanced reaction, answer parts a, b, c, and d. (Not all choices will be used) a) Balance the following reaction. Please place "1" if the coefficient is 1. HBO2 b) How many moles of water are produced from 3.50 moles of B;Hg react with excess O2? 3.50 mol B,Hs 3 mol O2 1 mol B2HS 3.50 mol B,H5 c) How many moles of water are produced from 19.2 g of B,Hg? 19.2 g B2HG 1 mol B2H6 27.67 g B2H6 2 mol H20 1 mol B2H6 1.39 mol H20
Given the following unbalanced reaction, answer parts a, b, c, and d. (Not all choices will be used) a) Balance the following reaction. Please place "1" if the coefficient is 1. HBO2 b) How many moles of water are produced from 3.50 moles of B;Hg react with excess O2? 3.50 mol B,Hs 3 mol O2 1 mol B2HS 3.50 mol B,H5 c) How many moles of water are produced from 19.2 g of B,Hg? 19.2 g B2HG 1 mol B2H6 27.67 g B2H6 2 mol H20 1 mol B2H6 1.39 mol H20
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Chemistry Problem: Balancing and Reaction Calculations**
Given the following unbalanced reaction, answer parts a, b, c, and d. (Not all choices will be used).
### a) Balance the following reaction. Please place “1” if the coefficient is 1.
B2H6 + O2 → HBO2 + H2O
\[ \boxed{1} \] B2H6 + \[ \boxed{3} \] O2 → \[ \boxed{2} \] HBO2 + \[ \boxed{2} \] H2O
### b) How many moles of water are produced from 3.50 moles of B2H6 react with excess O2?
\[ \boxed{\text{3.50 mol B2H6}} \] + \[ \boxed{\text{3 mol O2}} \] → \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{3.50 mol B2H6}} \]
### c) How many moles of water are produced from 19.2 g of B2H6?
\[ \boxed{\text{19.2 g B2H6}} \] + \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{27.67 g B2H6}} \]
\[ \boxed{\text{2 mol H2O}} \] = \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{1.39 mol H2O}} \]
### d) What mass of O2 will be needed to burn 36.1 g of B2H6?
\[ \boxed{\text{36.1 g B2H6}} \] + \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{27.67 g B2H6}} \]
\[ \boxed{\text{3 mol O2}} \] = \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{31.998 g O2}} \]
#### Answer choices:
\[ \boxed{1} \]
\[ \boxed{\text{125.2 g O2}} \]
\[ \boxed](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8356db49-748d-4110-bae4-35e11d46b97f%2F50e65157-dc38-4f45-a3bc-cc5b8dd4c280%2Fpfum9i_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemistry Problem: Balancing and Reaction Calculations**
Given the following unbalanced reaction, answer parts a, b, c, and d. (Not all choices will be used).
### a) Balance the following reaction. Please place “1” if the coefficient is 1.
B2H6 + O2 → HBO2 + H2O
\[ \boxed{1} \] B2H6 + \[ \boxed{3} \] O2 → \[ \boxed{2} \] HBO2 + \[ \boxed{2} \] H2O
### b) How many moles of water are produced from 3.50 moles of B2H6 react with excess O2?
\[ \boxed{\text{3.50 mol B2H6}} \] + \[ \boxed{\text{3 mol O2}} \] → \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{3.50 mol B2H6}} \]
### c) How many moles of water are produced from 19.2 g of B2H6?
\[ \boxed{\text{19.2 g B2H6}} \] + \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{27.67 g B2H6}} \]
\[ \boxed{\text{2 mol H2O}} \] = \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{1.39 mol H2O}} \]
### d) What mass of O2 will be needed to burn 36.1 g of B2H6?
\[ \boxed{\text{36.1 g B2H6}} \] + \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{27.67 g B2H6}} \]
\[ \boxed{\text{3 mol O2}} \] = \[ \boxed{\text{1 mol B2H6}} \] = \[ \boxed{\text{31.998 g O2}} \]
#### Answer choices:
\[ \boxed{1} \]
\[ \boxed{\text{125.2 g O2}} \]
\[ \boxed
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