According to the reaction,
2 moles of C4H10 give 10 moles of water
2×58 = 116 g C4H10 give 10×18 = 180 g water
61.55 g C4H10 give 180×61.55/116 g water
= 95.51 g water
Percent yield of water= mass obtained×100/ theoretical yield
= 43.21×100/95.51
= 45.24%
The balanced equations for the combustion of butane (C4H10.58.124 gmollis: 2C4H10 + 1302 —> 8CO2 +...
14. (4 pts.) Butane (C4H10) reacts with oxygen (O2) according to the reaction: 2C4H10(g)+1302 (g) 8CO2(g) +10H20 (l) A 4.00 L container is filled with 0.750 atm butane (C4H10). What pressure of O2 must be added to the container to react with butane? a. 137 pts anictdo noitssdsgnimoho eiadW To What would be the total pressure of the container after the O2 has been added? b.
Consider the following balanced equation: 13O2(g) + 2C4H10(g) → 8CO2(g) + 10H2O(l) If 3.78×102 grams of O2(g) reacts with an excess of C4H10(g), what is the theoretical yield of CO2(g) in moles?
Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atm and 23 ∘C, what is the volume of carbon dioxide formed by the combustion of 3.40 g of butane?
2C4H10 + 1302 → 8C02 + 10H20 In the combustion reaction above, butane (C.H..) reacts with Oxygen to form Co, and H20. If 5.00 moles of CO, were produced during the reaction, how many molecules of butane would have consumed during this reaction? 3.01 x 10-24 • 6.022 x 10^23 8.00 7.53 x 10^23
Part B Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10 (9) + 1302 (9) -8C02 (9) + 10H2O (1) At 1.00 atm and 23°C, what is the volume of carbon dioxide formed by the combustion of 1.00 g of butane? Express your answer with the appropriate units. View Available Hint(s) volume of CO2 = Value Units Submit
Question 25 2 pts Butane releases heat when it burns. 2C4H10(g) + 1302(g) → 8C02(g) + 10H2O(1) AHrxn=-5754 kJ How much heat would be released if 0.171 mol of butane (C4H10)is combusted? Your answer should have 3 significant figures. Question 26 2 pts Name 3 ions that have the condensed electron configuration equal to Ne. Input the answers with the symbol and charge with no space between-for example, H+ or Ba2+.
Question 25 2 pts Butane releases heat when it burns. 2C4H10(g) + 1302(g) → 8C02(g) + 10H2O(1) AHrxn=-5754 kJ How much heat would be released if 0.171 mol of butane (C4H10)is combusted? Your answer should have 3 significant figures. Question 26 2 pts Name 3 ions that have the condensed electron configuration equal to Ne. Input the answers with the symbol and charge with no space between-for example, H+ or Ba2+.
- Butane (C4H20) reacts with oxygen (O2) according to the reaction: 2C4H10(g) + 1302(g) → 8C02(g) + 10H2O(l) L container is filled with butane to a pressure of 0.650 atm at 35°C. Oxygen is then added until the total pressure of the container reaches 1.5 atm. a. What is the partial pressure of Oxygen? b. How many moles of Butane were added to the container? C. Which reactant will limit the amount of CO2(g) formed in the reaction?
Butane, C4H10, is used for heating homes not served by natural gas. 2C4H10(l) + 13O2(g) → 8CO2(g) + 10H2O(l) H= − 2511.18kJ If 2003 kJ of heat is evolved, how many grams of water were produced?
14. (4 pts.) Butane (C4H10) reacts with oxygen (O2) according to the reaction: 2C4H10(g) + 1302(g) → 8C02(g) + 10H20(1) A4.00 L container is filled with 0.750 atm butane (CH2o). a. What pressure of Oz must be added to the container to react with butane? b. What would be the total pressure of the container after the O, has been added?