Liquid nitroglycerin, a very powerful explosive, has the formula C3H5(NO3)3. It is unstable and decomposes to...
Liquid nitroglycerin, a very powerful explosive, has the formula C3H5(NO3)3. It is unstable and decomposes to form carbon dioxide, nitrogen, water, and oxygen. a. Write the balanced chemical equation for this decomposition. Write the starting materials on the left and the products on the right side of the arrow. HINT: Don’t forget the diatomic molecules! b. How many grams of carbon dioxide are formed from 10.00 grams of liquid nitroglycerin? Use significant figures and show your work.
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Liquid nitroglycerin, a very powerful explosive, has the formula
C3H5(NO3)3. It is unstable and decomposes to...
Balance the equation for explosive reaction of nitroglycerin, C3H5(NO3)3, Then assign oxidation numbers to each element,...
Balance the equation for explosive reaction of nitroglycerin, C3H5(NO3)3, Then assign oxidation numbers to each element, by writing it above each element in your chemical equation. The products formed are carbon dioxide, nitrogen, water and oxygen
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The...
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (CzH,(NO3),) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide X 2. Suppose 36.0 L of carbon...
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The...
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin ( C3H5NO33 ) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 37.0L of carbon...
Nitroglycerin is a powerful explosive that forms four different gases when it decomposes (i.e. when it...
Nitroglycerin is a powerful explosive that forms four different gases when it decomposes (i.e. when it explodes) as shown in the equation below. Calculate the volume in mL of nitrogen gas that will be collected at 1.25 atm and 112°C by the decomposition of 12.8 g of nitroglycerin, C3H5(NO3)3. Use the correct SF and units. 4 C3H5(NO3)3 (1) -->6 N2(g) + O2 (g) + 12 CO2 (g) + 10 H20 (g)
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The...
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin ( C 3 H 5 NO 3 3 ) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon...
Trinitroglycerin, C3H5N3O9 (usually referred to simply as nitroglycerin), has been widely used as an explosive. Alfred...
Trinitroglycerin, C3H5N3O9 (usually referred to simply as nitroglycerin), has been widely used as an explosive. Alfred Nobel used it to make dynamite in 1866. Rather surprisingly, it also is used as a medication, to relieve angina (chest pains resulting from partially blocked arteries to the heart) by dilating the blood vessels. At 1 atm pressure and 25 °C, the enthalpy of decomposition of trinitroglycerin to form nitrogen gas, carbon dioxide gas, liquid water, and oxygen gas is –1541.4 kJ/mol. One...
Show all work please A student in the chemistry lab reacted liquid hexane (C_6H_14) with oxygen...
Show all work please
A student in the chemistry lab reacted liquid hexane (C_6H_14) with oxygen of the air to produce carbon dioxide gas and liquid water. Write a balanced chemical equation for the reaction How many O_2 molecules are required to react completely with 48.8 g of C_6H_14? How many grams of carbon dioxide are produced from 48.8 g of C_6H_14? Determine the amount of Cu_3P formed if 175 grams of copper is reacted with 35.0 grams of P4....
A. Classify each of the following reactions as decomposition, combination, combustion, 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g) 2KClO3(s)→2KCl(s)+3O2(g) S(s)+3F2(g)→SF6(g) CaO(s)+H2O(l)→Ca(OH)2(aq) 2Cu(NO3)2(s)→2CuO(s)+4NO2(g)+O2(g)...
A. Classify each of the following reactions as decomposition, combination, combustion, 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g) 2KClO3(s)→2KCl(s)+3O2(g) S(s)+3F2(g)→SF6(g) CaO(s)+H2O(l)→Ca(OH)2(aq) 2Cu(NO3)2(s)→2CuO(s)+4NO2(g)+O2(g) B. Solid aluminum metal and diatomic chlorine gas react spontaneously to form a solid product. Give the balanced chemical equation (including phases) that describes this reaction. Indicate the phases using abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Express your answer as a chemical equation. C. When heated, solid copper(II) carbonate decomposes to solid copper(II) oxide and carbon dioxide gas. Give...
A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a...
A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a "1" if necessary. Identify the type of reaction in the right column. Balanced Equation Type of Reaction 1. H.As2O7 → _ As2O3 + _H20 2. _N2+_02—_N20 _NaI + _Br2 → _NaBr +_12 PbCrO4 +_HNO3 → __Pb(NO3)2 + __H2CrO4 . _C3H8 +_02 → __CO2 + __H20 TiCl4 + _ Mg → _ MgCl2 + ____Ti CuSO4 +_ KCN → ___Cu(CN)2 +_K2SO4 Ca(ClO3)2 → _ CaCl2...
1. Calculate the number of moles in each sample. a. 15.7 g CCl b. 1.8 x...
1. Calculate the number of moles in each sample. a. 15.7 g CCl b. 1.8 x 1021 formula units of NaC 2. Calculate the number of grams in each sample 1.23 mol magnesium bromide 7.310 x 1025 molecules of H202 a. b. 3. Calculate the mass percent of H in each of the following compounds. C2H2 C2HsCI a. b. 4. Calculate the empirical formula of each of the following Methy butyrate: 58.80 % C, 9.87 % H, 31.33 % O...
Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (CzH,(NO3),) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide X 2. Suppose 36.0 L of carbon...
Nitroglycerin is a powerful explosive that forms four different gases when it decomposes (i.e. when it explodes) as shown in the equation below. Calculate the volume in mL of nitrogen gas that will be collected at 1.25 atm and 112°C by the decomposition of 12.8 g of nitroglycerin, C3H5(NO3)3. Use the correct SF and units. 4 C3H5(NO3)3 (1) -->6 N2(g) + O2 (g) + 12 CO2 (g) + 10 H20 (g)
Show all work please
A student in the chemistry lab reacted liquid hexane (C_6H_14) with oxygen of the air to produce carbon dioxide gas and liquid water. Write a balanced chemical equation for the reaction How many O_2 molecules are required to react completely with 48.8 g of C_6H_14? How many grams of carbon dioxide are produced from 48.8 g of C_6H_14? Determine the amount of Cu_3P formed if 175 grams of copper is reacted with 35.0 grams of P4....
A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a "1" if necessary. Identify the type of reaction in the right column. Balanced Equation Type of Reaction 1. H.As2O7 → _ As2O3 + _H20 2. _N2+_02—_N20 _NaI + _Br2 → _NaBr +_12 PbCrO4 +_HNO3 → __Pb(NO3)2 + __H2CrO4 . _C3H8 +_02 → __CO2 + __H20 TiCl4 + _ Mg → _ MgCl2 + ____Ti CuSO4 +_ KCN → ___Cu(CN)2 +_K2SO4 Ca(ClO3)2 → _ CaCl2...
1. Calculate the number of moles in each sample. a. 15.7 g CCl b. 1.8 x 1021 formula units of NaC 2. Calculate the number of grams in each sample 1.23 mol magnesium bromide 7.310 x 1025 molecules of H202 a. b. 3. Calculate the mass percent of H in each of the following compounds. C2H2 C2HsCI a. b. 4. Calculate the empirical formula of each of the following Methy butyrate: 58.80 % C, 9.87 % H, 31.33 % O...
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