1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C,H,(NO,).) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 30.0 L of carbon dioxide gas are produced by this reaction, at a 15.0 °C and pressure of exactly 1 atm. Calculate the mass of temperature of nitroglycerin that must have reacted. Be sure your answer has the correct number of significant digits.

21 Consider the combustion of in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. C₅H₈ (l) + 7 O₂ (g) → 5 CO₂ (g) + 4 H₂O (g) d If 4790 J of heat were absorbed by the water, then how much heat, in J, was produced by the combustion of C₅H₈? (include the appropriate sign)

Magnesium will burn in air to form both Mg3N2 and MgO. What mass of each product would be found if burning a 3.28 g sample of magnesium to completion produces a combined total of 5.09 g of the two products?  g Mg3N2  g MgO

Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO3) into solid calcium oxide and gaseous carbon dioxide. x10 2. ose 20.0 L of carbon dioxide gas produced by this reaction, at a temperature of 370.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.

Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO,) into solid calcium oxide and gaseous carbon dioxide. ? 2. Suppose 11.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 360.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.

Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO2) into solid calcium oxide and gaseous carbon dioxide. C 2. Suppose 86.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 260.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.

When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC.  After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 107.87 grams.  For this problem, assume the  specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures.  What is the heat transferred by this reaction, in Joules?