Question

From the reaction: B2H6 + O2 → HBO2 + H2O a. What mass of O2 will...

From the reaction: B2H6 + O2 → HBO2 + H2O

a. What mass of O2 will be needed to burn 36.1 g of B2H6?

b. What mass of B2H6 will you need to produce 10g of HBO2, if this reaction has an experimental yield of 45%?         

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
C6H6 + O2  →  CO2 + H2O If at the beginning of the reaction you used 9.92 g...
C6H6 + O2  →  CO2 + H2O If at the beginning of the reaction you used 9.92 g C6H6 and 9.85 g O2, what is the theoretical yield (in grams) of H2O? (you will need to find the limiting reagent and then the theoretical yield of H2O from this reagent)
Consider the reaction of butane, C4H10, with O2 to produce CO and H2O. If you react...
Consider the reaction of butane, C4H10, with O2 to produce CO and H2O. If you react 110 g of butane with 240 g of O2 and produce 140 g of CO, what is the percent yield for the reac/on?
Diborane (B2H6) reacts with water to form boric acid (H3BO3) and hydrogen gas (H2) according to...
Diborane (B2H6) reacts with water to form boric acid (H3BO3) and hydrogen gas (H2) according to the following reaction: B2H6(g) + 6H20(L)----> 2H3BO3(s)+ 6H2(g) [Molar Masses (g/mol): B2H6:27.67, H2O: 18.02, H3BO3: 61.83, H2:2.02] a.) In a particular experiment 18.0 mol of H2O are consumed, how many mol of H3BO3 were produced? b.) Calculate the mass (in g) of B2H6 needed to produce 278.2g of H3BO3 (assuming excess H2O)
Consider the reaction of C3H8 with O2 to form CO2 and H2O. If 4.21 g O2...
Consider the reaction of C3H8 with O2 to form CO2 and H2O. If 4.21 g O2 is reacted with excess C3H8 and 2.46 g of CO2 is ultimately isolated, what is the percent yield for the reaction?
Consider the following chemical reaction: 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.6 L...
Consider the following chemical reaction: 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.6 L of O2 at a temperature of 305 K and a pressure of 0.951 atm ? m=?? g
Consider the following chemical reaction. 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.4 L...
Consider the following chemical reaction. 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.4 L of O2 at a temperature of 335 K and a pressure of 0.965 bar ?
1) Tungsten (W) reacts with Cl2 to form WCl6. What mass of WCl6 is formed from...
1) Tungsten (W) reacts with Cl2 to form WCl6. What mass of WCl6 is formed from the reaction of 12.6 g W with 13.6 g Cl2? 2) NH3 reacts with O2 to produce NO and H2O. How many moles of O2 are needed to react with exactly 10.0 moles of NH3?
Consider the following chemical reaction: 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.5 L...
Consider the following chemical reaction: 2H2O(l)→2H2(g)+O2(g) What mass of H2O is required to form 1.5 L of O2 at a temperature of 325 K and a pressure of 0.946 atm ? Express your answer using two significant figures.
Gaseous methane CH4 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and...
Gaseous methane CH4 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . Suppose 5.3 g of methane is mixed with 36.1 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.
Consider the reaction:   2 H2 + O2   → 2 H2O What if 3.0 mol H2 and...
Consider the reaction:   2 H2 + O2   → 2 H2O What if 3.0 mol H2 and 2.0 mol O2 were allowed react. The limiting reactant is ______. Complete consumption of the limiting reactant would mean the consumption of _____ mol of the other reactant; _____ mol of excess reactant would remain unreacted if the reaction went to completion. The theoretical yield is ____ mol or ____ g of _____. What if only 2.85 mol of product was obtained? Then, we...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT