Here is the equation 2 C 4 H 10 (g)+13 O 2 (g)→10 H 2 O(g)+8C...

Here is the equation 2 C 4 H 10 (g)+13 O 2 (g)→10 H 2 O(g)+8C O 2 (g) Calculate the mass of water produced when 1.20 g of butane reacts with excess oxygen. Calculate the mass of butane needed to produce 68.0 g of carbon dioxide.

Expert Solution

1)

2 C4H10 + 13 O2 ------------------------> 10 H2O + 8 CO2

116 g 180 g

1.20 g ?

mass of water produced = 180 x 1.20 / 116

= 1.86 g

mass of water produced = 1.86 g

2)

2 C4H10 + 13 O2 ------------------------> 10 H2O + 8 CO2

116 g 352 g

? 68.0 g

mass of butane = 116 x 68 / 352

= 22.4 g

mass of butane = 22.4 g

queen_honey_blossom answered 1 year ago

The thermal decomposition of dimethyl ether CH 3 2 O g CH 4 g H 2...

The thermal decomposition of dimethyl ether CH 3 2 O g CH 4 g H 2 g CO g is to be carried out in an isothermal 2.00-liter laboratory reactor at 600°C. The reactor is charged with pure dimethyl ether at a pressure of 350 torr. After about two hours, the reactor pressure is 875 torr. (a) Has the reaction proceeded to completion at the end of the two-hour period? If not, what percentage of the dimethyl ether has decomposed?...

Calculate the ΔH for the reaction. 2 C (s) + 3 H2 (g) + 1/2 O2...

Calculate the ΔH for the reaction. 2 C (s) + 3 H2 (g) + 1/2 O2 (g) = C2H5OH (l) Given the following information: C (s) + O2 (g) = CO2 (g) ΔH = -393.5 KJ/mole 2 H2 (g) + O2 (g) = 2 H2O (l) ΔH = -571.6 KJ/mole C2H5OH (l) + 3 O2 (g) = 2 CO2 (g) + 3 H2O (l) ΔH = -1367.5 KJ/mole

A compound is composed of only C, H, and O. The combustion of a 0.519-g sample...

A compound is composed of only C, H, and O. The combustion of a 0.519-g sample of the compound yields 1.24g of CO2 and 0.255g of H2O. What is the empirical formula of the compound?

A 49.5 g sample of a substance which contains C, H, and O is burned in...

A 49.5 g sample of a substance which contains C, H, and O is burned in excess oxygen, producing 110.0 g of CO2 and 22.5 g of H2O. A mass spectrum confirms that the molar mass of the sample is 162.0 g/mol. a.) how many moles and grams of carbon were in the original sample? b.) How many moles and grams of hydrogen were in the original sample? c.) How many moles and grams of oxygen were in the original...

An unknown compound contains only C , H , and O . Combustion of 6.50 g...

An unknown compound contains only C , H , and O . Combustion of 6.50 g of this compound produced 15.9 g CO2 and 6.50 g H2O . What is the empirical formula of the unknown compound? Insert subscripts as needed. empirical formula:[CHO]

Which of the following bonds are polar: C-Se, C-O, Cl-Cl, O=O, N-H, C-H? In the bond...

Which of the following bonds are polar: C-Se, C-O, Cl-Cl, O=O, N-H, C-H? In the bond or bonds that you selected, which atom has the greater electronegativity?

0.6908 g of an organic compound containing only C, H, and O was burned in excess...

0.6908 g of an organic compound containing only C, H, and O was burned in excess of pure O2, producing 1.7604 g of CO2 and 0.4504 g of H2O. 6.a) Calculate the number of grams of C and H in the combustion products and therefore in the 0.6908 g of the compound. Also calculate the number of grams of O in the 0.6908 g. Show your work. 6.b) What is the empirical formula of this compound?

when 1.6038 g of an organic iron compound Fe, C, H and O was burned in...

when 1.6038 g of an organic iron compound Fe, C, H and O was burned in O2, 2.9998 g of CO2 and 0.85850 g of H2O were produced. In a separate experiment to determine the mass percent of iron, 0.2726 g of the compound yielded 0.06159 g of Fe2O3. What is the empirical formula of the compound?

An unknown compound contains only C, H, and O. Combustion of 3.50 g of this compound...

An unknown compound contains only C, H, and O. Combustion of 3.50 g of this compound produced 7.96 g of CO2 and 3.26 g of H2O.What is the empirical formula of the unknown compound?

An organic compound contains C, H, N, and O. Combustion of 0.3069 g of the compound...

An organic compound contains C, H, N, and O. Combustion of 0.3069 g of the compound produces 0.8301 g CO2 and 0.2975 g H2O. A sample of 0.5322 g of the compound was analyzed for nitrogen. At STP, 30.54 mL of dry N2 (g) was obtained. In a third experiment, the density of the compound as a gas was found to be 3.68 g/L at 143 deg C and 244 torr. Calculate the empirical formula and the molecular formula of...

Question