xtullyx16
09-26-2010, 06:59 PM
Yet again critical thinking worksheet is giving me fits! More fits than last time atleast!
#1
Gaseous Butane (C4H10) is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 5.00mL butane ( density = .579 g/mL)
A. Write and balance the combustion reaction of butane.
2 (C4H10) + 13 O2 ------> 8 CO2 + 10 H20
B. How many grams of oxygen are needed to burn the butane completely?
C. How many moles of CO2 form when all the butane burns?
D. How many total molecules of gas form when the butane burns completely?
#2
Sodium borohydride (NaBH4, sold commercially as a detergent called Borax) is used industrially in many organic syntheses. One way to prepare it is by reacting sodium hydride with gaseous diborane (B2H6). Assuming a 95.5% yield, how many grams of NaBH4 can be prepared by reacting 7.88g of sodium hydride and 8.12g of diborane?
#1
Gaseous Butane (C4H10) is compressed and used as a liquid fuel in disposable cigarette lighters and lightweight camping stoves. Suppose a lighter contains 5.00mL butane ( density = .579 g/mL)
A. Write and balance the combustion reaction of butane.
2 (C4H10) + 13 O2 ------> 8 CO2 + 10 H20
B. How many grams of oxygen are needed to burn the butane completely?
C. How many moles of CO2 form when all the butane burns?
D. How many total molecules of gas form when the butane burns completely?
#2
Sodium borohydride (NaBH4, sold commercially as a detergent called Borax) is used industrially in many organic syntheses. One way to prepare it is by reacting sodium hydride with gaseous diborane (B2H6). Assuming a 95.5% yield, how many grams of NaBH4 can be prepared by reacting 7.88g of sodium hydride and 8.12g of diborane?